A 17 mL solution of 15 mM sodium iodate is titrated by precipitation with 10 mM lead (II) acetate...
Question:
A 17 mL solution of 15 mM sodium iodate is titrated by precipitation with 10 mM lead (II) acetate ({eq}Pb(CH_3CO_2)_2 {/eq}). Determine the concentrations of lead and iodate free in solution at each titration volume listed below.
a) 5 mL before the equivalence point
b) At the equivalence point
c) 6 mL past the equivalence point
Precipitation Reaction:
The formation of a stable solid compound in the final solution when the two or more aqueous ionic compounds are mixed together is known as the precipitation reaction. It is also known as ion exchange reaction.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerWe are given:
- Molarity of {eq}\rm NaIO_3 = 15\ mM {/eq}
- Volume of {eq}\rm NaIO_3 = 17\ mL {/eq}
- Molarity of {eq}\rm Pb(CH_3CO_2)_2 = 10\ mM {/eq}
...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
What is Precipitation? - Definition, Types & Formation
from
Chapter 19 / Lesson 8
53K
What is precipitation? Learn the definition, formation, types, and examples of precipitation. Also, learn the meaning of the term precipitate.
Related to this Question
- If 38.5 mL of lead (II)nitrate solution reacts completely with excess sodium iodide solution to yield .628g of precipitate, what is the molarity of lead (II) ion in the original solution?
- What is the concentration of lead ions in a solution if they are completely precipitated from 36.3 mL of solution by 29.6 mL of 0.35M potassium iodide.
- In the laboratory, you dissolve 24.4 g of sodium iodide in a volumetric flask and add water to a total volume of 250 mL. a) What is the molarity of the solution? b) What is the concentration of the sodium cation? c) What is the concentration of the io
- In the laboratory, you dissolve 22.8 g of copper(II) acetate in a volumetric flask and add water to a total volume of 250 ml. (a) What is the molarity of the solution? (b) What is the concentration of the copper(II) cation? (c) What is the concentrati
- A chemist must prepare 975 mL of a 160 mM aqueous sodium carbonate solution. He will do this by pouring out some 0.174 mol/L aqueous sodium carbonate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume of th
- The concentration of SO42-(aq) in a sample of river water can be determined using a precipitation titration in which a salt of Ba2+(aq) is the standard solution and BaSO4(s) is the precipitate formed. What is the concentration of SO42-(aq) in a 55.7-mL sa
- Suppose 7.17 g of barium acetate is dissolved in 350 mL of a 79.0 mM aqueous solution of sodium chromate. Calculate the final molarity of barium cation in the solution. You can assume the volume of the solution doesn't change when the barium acetate is di
- In the laboratory you dissolve 14.0 g of iron(II) acetate in a volumetric flask and add water to a total volume of 125 mL. A) What is the molarity of the solution? B) What is the concentration of the iron(II) cation? C) What is the concentration of the ac
- Determine the concentrations of Na_2CO_3, Na , and CO_3^{2-} in a solution prepared by dissolving 2.22 \times 10^4 g Na_2CO_3 in 2.25 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species
- What is the molarity of a solution made by dissolving 6.79 g of sodium acetate in water and diluting to 750 mL? (Molar mass of NaC2H3O2 is 82.0 g/mol.)
- Suppose 1.12 g of barium acetate is dissolved in 100 mL of a 63.0 mM aqueous solution of sodium chromate. Calculate the final molarity of barium cation in the solution. You can assume the volume of the solution doesn't change when the barium acetate is di
- What is the molarity of a solution made by dissolving 5.69 g of sodium acetate in water and diluting to 750 mL? (The molar mass of NaC_2H_3O_2 is 82.0 \dfrac{g}{mol}.)
- Calculate the molar concentration of a sodium acetate solution prepared by diluting 45.0 mL of a solution containing 25.0 ppm sodium acetate (Na2C2H3O2) to a total of 0.500 liters of solution. Assume
- In the laboratory, you dissolve 22.8 g of copper(II) acetate in a volumetric flask and add water to a total volume of 250 mL. (a) What is the molarity of the solution? (b) What is the concentration of the copper(II) cation? (c) What is the concentrat
- Determine the concentrations of Na_2CO_3, Na^+, and CO_3^{2-} in a solution prepared by dissolving 1.85 times 10^{-4} g Na_2CO_3 in 2.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic specie
- In the laboratory, you dissolve 13.0 g of copper(II) acetate in a volumetric flask and add water to a total volume of 375 mL. a. What is the molarity of the solution? b. What is the concentration of the copper(II) cation? c. What is the concentration of t
- A solution is 0.0010 M in each of the metal cations Fe^{+2} and Hg^{+2} (Fes: K_{SPA}= 6 times 10^2; HgS: K_{SPA} = 2. 2 times 10^-22) What is the iodate concentration in the 4.00 mL of saturated copper iodate solution?
- What is the concentration of a ( KIO3 ) potassium iodate solution after you complete the following procedure: Pipette 10 mL of a 0.31 M KIO_3 stock solution to a 100 mL volumetric flask and then add w
- In the laboratory, you dissolve 16.1 g of sodium iodide in a volumetric flask and add water to a total volume of 500 mL. a. What is the molarity of the solution? b. What is the concentration of the sodium cation c. What is the concentration of the
- In the laboratory you dissolve 22.3 g of iron(II) iodide in a volumetric flask and add water to a total volume of 5000 mL. A. What is the molarity of the solution? B. What is the concentration of the iron(II) cation? C. What is the concentration of
- To 50.00 mL of 0.400 M CaBr2(aq) is added 100.00 mL of 0.200 M CaCl2(aq) and 100.00 mL of 0.100 M Na3PO4(aq) . Determine the mass of precipitate which forms, as well as the molarity of each ion in the resulting solution. Assume the individual volumes are
- Suppose 14.3 g of lead (II) acetate is dissolved in 300 mL of a 0.40 M aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the lead (II) acetate
- A 500.0 ml sodium iodide (NaI) solution contains 31.7g of Nal. What is the molar concentration of the solution?
- Titration with solutions of potassium bromate, K B r O 3 , can be used to determine the concentration of A s ( I I I ) . What is the molar concentration of A s ( I I I ) in a solution if 21.90 mL of 0.120 M K B r O 3 is needed to titrate 51.65 mL o
- By pipet, 8.00 mL of a 0.823 M stock solution of potassium permanganate (KMnO4) was transferred to a 50.00 mL volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.
- A solution was prepared by dissolving 0.450 g MgSO_4 (FW = 120.363 g / mol) in 0.500 L of water. A 50.0 mL aliquot of this solution consumed 37.60 mL of EDTA solution in a titration. How many milligrams of CaCO_3 (FW = 100.089 g / mol) will react with 1.0
- In the laboratory you dissolve 18.1 g of chromium(II) acetate in a volumetric flask and add water to a total volume of 125 mL. What is the molarity of the solution? M. What is the concentration of the
- Calculate the molarity of a solution prepared by dissolving 0.170 moles of potassium iodide (KI) in enough water to make 250.0 mL of KI solution.
- 1) In the laboratory, you dissolve 23.1 g of sodium carbonate in a volumetric flask and add water to a total volume of 500 mL. a) What is the molarity of the solution? b) What is the concentration o
- A 25.00-mL aliquot of Na2C2O4(aq) with an unknown concentration is titrated with 0.1435 M HCl(aq). The equivalence point is reached at a volume of 18.35 mL. What is the concentration (in M) of the Na2C2O4(aq) solution?
- If 45.1 mL of a solution containing 8.30 g of silver nitrate is added to 31.3 mL of 0.511 M sodium carbonate solution, calculate the molarity of silver ion in the resulting solution. (Assume volumes are additive.)
- I have a 17.0 % by mass solution of sodium acetate, CH_3COONa (MM = 82.0 g / mol) in water (MM = 18.02 g / mol). What is the molarity of this solution? The density of the solution is 1.09 g / mL.
- Suppose 0.160 g of ammonium acetate is dissolved in 50.0 mL of a 33.0 mM aqueous solution of sodium chromate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume
- The concentration of Ca2+ in an unknown solution was determined by titration with the EDTA solution standardized at 5.231 x 10-4 M. In the determination, 25.00 mL of the unknown solution was diluted to 250.00 mL with deionized water. A 25.00 mL aliquot of
- Suppose 3.96g of sodium acetate is dissolved in 200. mL of a 0.10 M aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the sodium acetate is di
- Determine the concentration of all ions present in the solution when 0.200 moles of sodium sulfate are dissolved in water to produce 50.0 mL of solution.
- In the laboratory, you dissolve 13.6 g of potassium hydroxide in a volumetric flask and add water to a total volume of 500 mL. a. What is the molarity of the solution? b. What is the concentration of the potassium cation? c. What is the concentration of t
- Calculate the concentrations of each ion present in a solution that results from mixing 13.7 mL of a 0.37 M NaClO3(aq) solution with 25.4 mL of a 0.64 M Na_2SO_4(aq). Assume that the volumes are addit
- A chemist makes 870 mL of barium acetate Ba(C2H3O2)2 working solution by adding distilled water to 250 mL of a 0.264 mol/L stock solution of barium acetate in water. Calculate the concentration of the chemist's working solution. (Round your answer to 3 si
- Consider a 640 mL solution containing 33.4 g of NaF and a 640 mL solution containing 210.1 g of BaF2. What are the molar concentrations of sodium, barium, and fluoride ions when the two solutions are mixed together?
- Suppose 0.795 g of sodium iodide is dissolved in 100. mL of a 39.0 m M aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of th
- A 25-mL aliquot of a 0.03816 M KIO3 solution is titrated to the stoichiometric point with 20.97 mL of sodium thiosulfate, Na2S2O3, solution. What is the molar concentration of the Na2S2O3 solution?
- Suppose 17.8 g of sodium iodide is dissolved in 150. mL of a 0.50 M aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the sodium iodide is dissol
- If a 100.0 mL solution containing Fe^{2+} ions is titrated with 15.2 mL of 0.135 M Cr_2O_7^{2-}, calculate the molar concentration of Fe^{2+} ions in the solution. Cr_2O_7^{2-}(aq)
- A chemist makes 340 mL of barium acetate (Ba(C_2H_3O_2)_2 working solution by adding distilled water to 30 mL of a 1.54 mol/L stock solution of barium acetate in water. Calculate the concentration of the chemist's working solution. Be sure your answer has
- A solution is made by dissolving 1.362 g of nickel(II) acetate in enough water to make 250.0 mL of solution. What is the molarity of this solution?
- A solution is prepared by dissolving 49.73 g of Na_2CO_3 in water to a total volume of 800.0 mL. Then, 5.00 mL of this solution was diluted with water to a total volume of 40.0 mL. What are the concentrations of each of the ions in the diluted solution?
- Calculate the formal concentration of a sodium acetate solution prepared by diluting 45.0 mL of a solution containing 25.0 ppm sodium acetate (NaC_2H_3O_2, FM=82.03 g/mol) to a total of 0.500 liters o
- A solution of FeSCN+2was prepared by taking 3000 L of a 0.500 0.005 M stock solution (measured with a P1000 micro pipet) and diluting it to 250.0 0.1 mL in a volumetric flask. Determine the final concentration and the uncertainty.
- The concentration of SO_4^{2-} (aq) in a sample of river water can be determined using a precipitation titration in which a salt of Ba^{2+} (aq) is the standard solution and BaSO_4 (s) is the precipi
- A solution of 220 mL of 0.200 M KOH is mixed with a solution of 120 mL of 0.240 M NiSO_4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3. Calculate the molarity of
- How many milliliters of a solution of 0.0013 M EDTA4- would be used to titrate the lead in 1000 mL of a 0.0073 M solution of Pb(NO3)2?
- Chloride in a brine solution is determined by a precipitation titration. A 10.00 mL aliquot of the solution is titrated with 15.00 mL of standard 0.1182 M AgNO3 solution. The excess silver is titrated
- If it takes 35.0 mL of 0.250 M Fe2+ to titrate 100 mL of a solution containing Cr2O72-, what is the molar concentration of Cr2O72-?
- A 0.5118 g sample of CaCO_3 is dissolved in concentrated HCl (12 M) the solution was diluted to 250 mL in a volumetric flask to obtain a solution for standardizing the EDTA titrant. How much molarity of the Ca^{2+} in the 250 mL of the solution?
- What is the molarity of a sodium acetate solution that consists of 4.1 grams of sodium acetate in 80 mL of water?
- If 0.135 g of CuCl2 is dissolved in 25.00 mL of water and titrated with 35.45 mL of Na2S2O3 solution (of unknown concentration) to reach the end point, what mass of copper atoms is present in the sample at the end of the titration?
- In the laboratory, you dissolve 19.3 g of calcium acetate in a volumetric flask and add water to a total volume of 375 ml. (a) What is the molarity of the solution? (b) What is the concentration of the calcium cation? (c) What is the concentration o
- A chemist prepares a solution of barium acetate by measuring out 14 g of barium acetate into a 300 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration (in mol/L) of the chemist's barium acetate solution.
- In a titration for the determination of the chloride ion, a solution of 0.1M AgNO_3 is used against a solution, the volume of which is 100 mL. At the completion of the titration, the residual concentrations of silver and chloride ions are equal and the to
- In the laboratory, you dissolve 13.2 grams of sodium bromide in a volumetric flask and add water to a total volume of 125 mL. a. What is the molarity of the solution? b. What is the concentration of the sodium cation? c. What is the concentration of the b
- A solution is prepared by dissolving 5.20 g of Al(NO3)3 in water to make 200.0 mL of solution. What are the molar concentrations of Al3+ ions and NO3- ions in this solution?
- A 25.00 mL sample of a lead ion solution gave 0.2375 g of lead chromate. What is the concentration on lead in the solution in mg/L?
- A 25.00 mL sample of a lead ion solution gave 0.2375 g of lead chromate. What is the concentration of lead in the solution in mg/L?
- A 15.0% by mass NaOH(aq) solution has a density of 1.1655 g/mL. What is the molar concentration of this solution?
- A 30.0 mL sample of a K O H solution of unknown concentration requires 11.6 mL of 0.200 M H 2 S O 4 solution to reach the end point in a titration. What is the molarity of the K O H solution?
- A 0.5118 g sample of CaCO_3 is dissolved in concentrated HCl (12 M) the solution was diluted to 250 mL in a volumetric flask to obtain a solution for standardizing the EDTA titrant. How many moles of Ca^{2+} is in a 25 mL aliquot of the solution?
- An IV bag is labeled as 0.800% w/w sodium iodide in water solution with a density of 1.014 g/mL. What is the concentration of sodium iodide in the solution expressed in molarity, molality, and mole fraction?
- You dissolve 346. mg of a compound (AwBxCyDz) in water producing 17.81 mL of solution and use the photometer and standard solutions to find that the concentration of the A is 1.18 x 10¯² M. The molar mass of A is 166.28 g/mol. What are the numbe
- Calculate each of the following quantities: (a) Grams of solute in 185.8 mL of 0.267 M calcium acetate. (b) Molarity of 500 mL of solution containing 21.1 g of potassium iodine. (c) Moles of solute in
- You have 75.0 mL of a 2.50 M solution of Na_2CrO_4(aq). You also have125 mL of a 2.50 M solution of AgNO_3(aq). Calculate the concentrations of the following ions when the two solutions are added together. Na_2CrO_4(aq) + 2AgNO_3(aq) longrightarrow A
- A chemist must dilute 67.6 mL of 321. mM aqueous potassium iodide KI solution until the concentration falls to 16. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters.
- Calculate the molarity of a solution made by adding 30.7 mL of concentrated potassium hydroxide (34.5 % by mass, density 1.46 g/mL) to some water in a volumetric flask, then adding water to the mark t
- A solution of sodium carbonate contains 1.06 g of Na2CO3 dissolved in 100 mL of water. Calculate its concentration in normality. (d = 2.54 g/mL)
- Determine the molarity of K+ ions in a solution prepared by mixing 54.1 mL of a 0.639 M KClO4 solution and 21.8 mL of 0.900 M K2SO4.
- 28 mL of 0.10 M HaI is added to 60 mL of 0.1 M Sr(OH)P_2. Determine the concentration of OH^- in the resulting solution.
- In the laboratory you dissolve 18.6 g of potassium carbonate in a volumetric flask and add water to a total volume of 500 mL. What is the molarity of the solution? M. What is the concentration of th
- In the laboratory you dissolve 17.7g of sodium fluoride in a volumetric flask and add water to a total volume of 125 mL. What is the molarity of the solution? What is the concentration of the sodium cation? What is the concentration of the fluoride anio
- What is the molarity of a solution made by dissolving 8.56 g of sodium acetate in water and diluting it to 750.0 mL?
- What is the molarity of a solution made by dissolving 9.28 g of sodium acetate in water and diluting it to 750.0 mL?
- a. If 6.73 g of Na_2CO_3 is dissolved in enough water to make 250.0 mL of solution, what is the molar concentration of the sodium carbonate? b. What are the molar concentrations of the Na^+ and CO_3^{2-} ions?
- A 25 mL aliquot of 0.0104 M KIO3 solution is titrated to the stoichiometric point with 17.27 mL of sodium thiosulfate, What is the molar concentration of Na2S2O3 solution?
- A titration was performed in which 56 ml of a 0.022 M HCl solution was used to titrate 50 ml of a Pb(NO_3)_2 solution. (a) What was the original concentration of the Pb(NO_3)_2? (b) How many grams o
- A solution was prepared by dissolving 447 mg of potassium sulfate (K2SO4) in 749 mL of water. Calculate: A) mmoles of K2SO4 in 50 mL of solution B) Should the concentration of K2SO4 be described with Formal? Why or why not? C) Concentration of K2SO4 (in m
- The following three solutions are mixed: 100.0 mL of 0.130 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 110.0 mL of 0.200 M Ba(CN)2. a. What ionic compounds will precipitate out of the solution? b. What is the molarity of each ion remaining in the solution, as
- What is the molarity (mol/L) of sodium (Na) in a solution containing 0.4 mole of Na^+ cation in 400 mL of an aqueous (water) solution?
- If 1.39 g of KMnO4(s) is dissolved to prepare a 500.0 mL solution, what is the molar concentration of the MnO4-1 anion in this solution?
- Calculate the number of moles of potassium iodate (KIO) that were present in the 5.00 ml aliquot of standard potassium iodate solution.
- Calculate the molar concentration of iodide ions in each aqueous solution a) 15g of potassium iodide dissolved in 200mL of solution b) 12g of calcium iodide dissolved in 180mL of solution
- Suppose 100.0 mL of 0.400 M CoCl2 solution is mixed with 100.0 mL of 1.600 M NaOH solution. Determine how many moles of precipitate forms and the molarity of each ion (including spectator ions) after the precipitation process is complete.
- 1. Use a stock solution of 0.0974 M sodium chloride. (All glassware used is volumetric --> ? sig. figs) a. What is the concentration of a new solution prepared by pipetting 20 mL of the stock solutio
- A solution is made by dissolving 29.8g of sodium chromate, Na2CrO4, in enough water to make exactly 250mL of solution. Calculate the concentration (molarity) of Na2CrO4 in mol/L (M).
- A chemist prepares a solution of potassium iodide (KI) by measuring out 370. mu mol of potassium iodide into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's potassium iodide
- A .600 g sample of CaCO_3 is dissolve in concentrated HCl (12M). The solution was diluted to 250 mL in a volumetric flask to obtain a solution for standardizing the EDTA titrant. 1. What is the molar
- Calculate the molarity of sodium carbonate in a solution prepared by dissolving 5.9 g in enough water to form 250 ml of solution.
- Determine the concentration of SO_4^{2-} ion in a sample of groundwater, 100.0 mL of the sample is titrated with 0.0250 M Ba(NO_3)_2, forming insluble BaSO_4. If 4.24 mL of the Ba(NO_3)_2 solution is
- If 25.0 mL of sodium nitrate solution (0.100 mol/L) is added to 10.0 mL of sodium carbonate solution (0.150 mol/L), what is the concentration of sodium ions in the resulting mixture? Assume the volume
- In the laboratory, you dissolve 19.3 g of calcium acetate in a volumetric flask and add water to a total volume of 375 mL. What is the concentration of the acetate anion in this solution?
- A solution is prepared by dissolving 5.10 g of Na2SO4 in water to make 200.0 mL of solution. What are the molar concentrations of Na+ ions and SO42- ions in this solution?
- Calculate each of the following quantities: a) Grams of solute in 185.8 mL of 0.267 M calcium acetate. b) Molarity of 500. mL of solution containing 21.1g of potassium iodine. c) Moles of solute in 145.6 L of 0.850 M sodium cyanide.
Explore our homework questions and answers library
Browse
by subject