# A 0.5118 g sample of CaCO_3 is dissolved in concentrated HCl (12 M) the solution was diluted to...

## Question:

A {eq}\displaystyle \rm 0.5118 \ g {/eq} sample of {eq}\displaystyle \rm CaCO_3 {/eq} is dissolved in concentrated {eq}\displaystyle \rm HCl \ (12 \ M) {/eq} the solution was diluted to {eq}\displaystyle \rm 250 \ mL {/eq} in a volumetric flask to obtain a solution for standardizing the EDTA titrant.

How many moles of {eq}\displaystyle \rm Ca^{2+} {/eq} is in a {eq}\displaystyle \rm 25 \ mL {/eq} aliquot of the solution?

## Molarity

The concentration of a solution can be expressed in molarity. Molarity can be calculated by dividing the moles of the substance divided by the total volume of the solution in liters.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerWe first need to determine the concentration of the stock solution in molarity.

{eq}\begin{aligned} Molarity\;&=\;\frac{moles\;Calcium}{L\;soln}\\ ...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 9 / Lesson 4Learn how to find the molarity of a solution or the moles of gas in a given volume using stoichiometry. See examples of calculating moles from molarity.

#### Related to this Question

- 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 CaCO_3 are used (MW=100.1)?
- 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?
- 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
- A 0.4505 g sample of CaCO3 was dissolved in the HCl and the resulting solution diluted to 25.00 mL in a volumetric flask. A 25.00 mL aliquot of the solution required 29.25 mL of EDTA solution for titr
- A solution was prepared by dissolving 0.450 g of MgSO4 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 mg of CaCO3 will react with 1.00 mL of the EDTA solution?
- A 0.4505g sample of CaCO_3 was dissolved in HCl and the resulting solution was diluted to 250ml in a volumetric flask. A 25 ml aliquot of the solution required 24.25 ml of an EDTA solution for the tit
- 1. A 0.5100 g sample of CaCO3 is dissolved in 12 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. a. How many moles of CaCO3 are used (M.W. = 100.1g/mol)? b. What is t
- A 0.512 g sample of CaCO_3, is dissolved in 12 M HCl and the mixture is diluted to 250 mL. a) How many moles of CaCO_3, are used? b) What is the [Ca^{2+}] in the 250 mL solution? c) How many moles of Ca^{2+} is in a 25 mL sample of the 250 mL soluti
- A 0.3205g sample of CaCO3 was dissolved in HCl and the resulting solution diluted to 250.ml in a volumetric flask. A 25 mL sample of the solution required 18.75mL of EDTA solution for titration to the
- A 0.5215 gram sample of CaCO_3 is dissolved in 12 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. How many moles of CaCO_3 are used?
- A 0.5215-gram sample of CaCO3 is dissolved in 12 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. How many moles of CaCO3 are used?
- A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A. Calculate the concentration of Ca+2 in the 250 mL solution. B. How many moles of Ca+2 are in a 25 mL sample
- A 0.4243 g sample of CaCO3 is dissolved in 12 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. How many moles of CaCO3 are used (formula mass = 100.1 g/mol)?
- In the titration of 25.00 mL of a water sample, it took 18.240 mL of 3.210x10-3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample.
- If you are titrating 25.00 mL of a 1.00 mg/mL CaCO3 solution, how many mL of 0.010 M EDTA solution will be required to reach the equivalence point?
- In a titration of a 31-mL water sample, it took 22.5 mL of 0.200 M EDTA to reach the endpoint. How many moles of EDTA is in 22.5 mL of 0.200 M EDTA?
- In the titration of 25.00 mL of a water sample, it took 19.290 mL of 3.765x 10-3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample.
- A 25.00-mL aliquot of a standard calcium solution (M = 0.0068; 0.3412 grams of CaCO3 was added to a 500 mL flask) was titrated with a previously prepared EDTA solution. In the titration, 32.55 mL of the EDTA solution was required to reach the end point. W
- 100mL of the water sample is titrated with 0.0200M EDTA solution. It takes 9.0mL to reach the endpoint. How many moles of EDTA are used in the titration?
- 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
- A 48.60 mL aliquot from a 0.510 L solution that contains 0.420 g of MnSO_4 (FW = 151.00 g/mole) required 39.1 mL of an EDTA solution to reach the end point in a titration. What mass (in milligrams) of CaCO_3 (FW = 100.09 g/mole) will react with 1.01 mL o
- Calculate the number of grams of CaCO3 present and convert to mg. The titration of 25.00 mL took 19.290 mL of 3.765x10-3 M EDTA solution to reach the endpoint.
- A student titrates a 50.0 mL sample of water with a 0.005920M EDTA solution. If the titration requires 10.05 mL of EDTA to reach the endpoint, what is the total concentration of Mg^{2+} and Ca^{2+} in the water sample in moles per liter?
- In the titration of 25.00 ml of a water sample, it took 20.740 ml of 4.305 x 10^{-3}M EDTA solution to reach the endpoint. Convert the number of ml of bottled water used in each sample titration to Liters. (enter your answer with 3 significant figures)
- In a titration of a 31-mL water sample, it took 22.5 mL of 0.200 M EDTA to reach the end point. Approximately how many total moles of Ca2+ and Mg2+ are present in the water sample?
- Convert the number of mL of bottled water used in each sample titration to liters. The titration of 25.00 mL took 19.290 mL of 3.765x10-3 M EDTA solution to reach the endpoint.
- A 0.2481 g sample of marble was dissolved in 100 mL, and a 10.00 mL aliquot of the solution was titrated to an end point with 23.56 mL of 0.01052 M EDTA solution. What is the molecular weight?
- Solution A is 3.15 M CaCl2. Suppose 110 mL of solution A is diluted to 500 mL of solution B. Then 45.0 mL of solution B is diluted to 335 mL of solution C. What is the concentration in moles per liter of solution C?
- If you have 25 mL of a standard 1 mg/mL CaCO_3 solution, how many mL of the 0.010 M solution do you expect to use in the titration?
- You use 1.0093 g of calcium carbonate to make your standard solution. It takes 22.33 mL of your EDTA solution to reach the endpoint when you titrate 25.00 mL of your standard calcium solution. What is the molarity of the EDTA solution? The molar mass of
- 25 mL of tap-water is titrated with 0.005 M EDTA. 7.95 mL of EDTA is required for the complete reaction. What is the molarity of that total water hardness in the 25 mL sample?
- A titration was performed to standardize an EDTA solution. Use the following data to calculate the molarity of the EDTA solution: 20.00 mL of a standard solution containing 0.02000 M Ca2+ required 22.
- If you have 25 mL of a standard 1 mg/mL CaCO_3 solution, how many milliliters of the 0.010 M solution do you expect to use in the titration?
- 23.02 mL of a 0.1930 \dfrac{mol}{L} EDTA solution is required to titrate a sample to the equivalence point. How many moles of divalent metal cations were in your sample?
- 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 15.00 mL sample of a standard solution containing 1 g of CaCO3/L required 8.45 mL of EDTA to fully complex the Ca present. Calculate the volume of EDTA stoichiometrically equivalent to 1.0 mg of CaC
- A 20.0 mL solution containing 0.250 M Ni^{2+} ion was titrated with 0.0500 M EDTA while the system was buffered at pH=4.00. Determine the volume of EDTA needed to reach the equivalence point.
- 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 22.93 mL of a 0.0410 mol/L EDTA solution is required to titrate a sample to the equivalence point. How many moles of divalent metal cations were in your sample?
- 05 mL of sample water needs 10.9 mL .01M EDTA solution. What is the accurate Hardness of the sample in CaCO_3 (mg/L)?
- What is the molarity of a solution prepared by dissolving 25.2 g CaCO_3 in 600 mL of a water solution?
- You have been tasked with determining the concentration of Ca2+ in an unknown solution of calcium carbonate (CaCO3). You titrate 50.0 ml of the unknown solution with 0.0250 M EDTA. It requires 16.85 m
- Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. The titration of 25.00 mL took 19.290 mL of 3.765x 10-3 M EDTA solution to reach the endpoint.
- A sample of 15.0 mL of 0.0500 M (NH_4)_2SO_4 is diluted to 100.0 mL in a volumetric flask. Then 6.00 mL of this solution is removed and diluted further to a total volume of 17.00 mL. What is the molarity of NH_4^+ in the final solution?
- Assuming that 0.5 grams of a 1.0 gram sample is CaCO_3, what should the concentration of HCl (M) be if you want to use 25.0 mL for the titration?
- A 0.512 g sample of CaCO3 is dissolved in 12 M HCI, and the mixture is diluted to 250 mL. What is the Ca2+ in the 250 mL solution?
- When 26 mL of a 375 mL stock solution containing 2.1 M CaCl2 is diluted to 103 mL, how many moles of Ca2+ are in the new solution?
- Suppose 14.48 mL of 1.161 M HC2H3O2 solution is diluted to 59.37 mL. How many moles of HC2H3O2 are in this solution?
- A 25.00 mL sample of seawater was titrated for total hardness, the combined concentrations of magnesium and calcium ion, using 12.60 mL of an EDTA solution that was 0.1000 M. Assuming that the stoichiometry of the reaction between EDTA and both the ions i
- From standardization, you determine your EDTA solution is 0.0115 M. It takes 25.11 mL of your EDTA solution to reach the endpoint when titrating 50.00 mL of your unknown. What is the ppm of calcium carbonate in the unknown? The molar mass of calcium ca
- A 48.30 mL aliquot from a 0.480 L solution that contains 0.360 g of MnSO4 (Fw = 151.00 g/mol) required 41.8 mL of an EDTA solution to reach the endpoint in a titration. What mass (in milligrams) of CaCO3 (FW = 100.09 g/mol) will react with 1.85 mL of the
- A 40.0 mL sample of Ca(OH)2 was titrated with 0.0704 m HCl. The volume of HCl needed to reach the equivalence point was 18.2 mL. What was the concentration of Ca2+ present in the original solution?
- When 26 mL of a 120 mL stock solution containing 3.23 M CaF_2 is diluted to 35 mL, how many moles of F^- are in the new solution?
- A sample of oxalic acid, H_2C_2O_4, weighing 1.200 g is placed in a 100.0-mL volumetric flask, which is then filled to the mark with water. What is the molarity of the solution?
- A 72.4g sample of oxalic acid, H2C2O4, was dissolved in 1.00L of solution. How would you prepare 1.00L of 0.135M H2C2O4 from this solution? __________ mL of the __________ M solution in a 1L volumetric flask, and dilute to 1.00
- You have 26.44 ml of 1.83 M HCl in a beaker. You dilute this acid with 40.08 ml of water. When you analyze the solution you find that the number of moles of HCl in the new solution is ____.
- A 50 mL sample containing Ni2+ was treated with 25 mL of 0.05 M EDTA to complex all the Ni2+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5 mL of 0.05 M Zn2+. What was the concentration of Ni2+ in the original solut
- How would you make 250 mL of a 15% EDTA solution? How much of the solution should be used to make 500 mL of a 0.1% EDTA solution?
- Compound A is provided as a 500 mm solution. If 12.5 mL is taken and added to 12.5 mL of water, how many moles (or millimoles / micromoles) are there per 0.1 mL of the diluted solution?
- 0.4250 g of the dried calcium carbonate was diluted to 500 ml and 50 ml of this solution required 46.83 ml of an unknown EDTA solution.
- How many grams of EDTA is needed to prepare a solution of 250mL of 0.010M (mol/L) EDTA? The molar mass of EDTA is 372.244 g/mol.
- When performing a titration, 23.65 mL of 1.25 M calcium carbonate was used to neutralize 9.68 mL of HCl. What is the concentration of the HCl solution?
- Assume that 50 ml of 0.01 M EDTA solution were added to 25 ml of Co solution and the excess EDTA required 20 ml of 0.005 M Mg solution.
- 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 molarity of the solution?
- A 1.500 g sample of solid CaCO3 is dissolved in 25.00 mL of 1.000 M HCl solution. The excess amount of HCl is titrated with 0.100 M NaOH solution. The endpoint of the titration required 23.40 mL of NaOH solution. What is the percent CaCO3 in the sample? C
- Calculate the volume of 0.0500 M EDTA needed to titrate the Ca in 0.1973 g of CaCO_3.
- Calculate the concentration of 17.0 ml of EDTA if you use 25.0 ml of 0.05 M Zn^2+.
- A solution of CaCl_2 is prepared by dissolving 1.004 g of the solid in approximately 30 ''mL'' of water. How many moles of CaCl_2 does this solution contain? Suppose this same CaCl_2 solution is adde
- When 26 mL of a 120 mL stock solution containing 3.23 M CaF2 is diluted to 35 mL, how many moles of F- are in the new solution?
- 1. A graduate measured out a 100 mL hard water sample and titrated it with 37.6 mL of 0.0100 M EDTA solution for a total hardness endpoint, and 29.3 mL of 0.0100 M EDTA solution for a calcium endpoint
- Suppose you dissolved 0.7500 g calcium chloride, dihydrate and impure, in distilled water, and the volume was elevated to 200.00 mL in a volumetric flask. A rate of 10.00 mL of the same consumed the titration 18.9 mL 0.0125 M EDTA using CALCON as an indic
- Before performing an analysis of calcium in a powdered cement sample with an EDTA titration, the EDTA must be standardized. A 50.0 mL known solution of 5.67 x 10-3 M Ca2+ required 38.10 mL of an unknown EDTA solution to reach its end point. Based on t
- When 15 mL of a solution containing .29 M Ca(OH)2 is diluted to 32 mL, a dilute solution is formed. What is the OH-concentration in 5 mL of the dilute solution?
- Suppose you have completed a titration of a water sample. Your average titre value is 20 mL,concentration of EDTA was 0.01 M and your aliquot of sample was 50mL. Calculate the total water hardness (as equivalent CaCO3 in ppm) of the water sample. HINT: re
- What is the concentration of a solution prepared by diluting 17.3 mL of a 2.25 M solution of hydrochloric acid to the mark using a 100-mL volumetric flask?
- A sample of 15.00 mL of 0.0500 M (NH_4)_2SO_4 is diluted to 100.00 mL in a volumetric flask. Then 6.00 mL of this solution is removed and diluted future to a total volume of 17.00 mL. What is the molarity of NH_4^+ in the final solution?
- If the endpoint is reached when 50.00 mL of a tap water sample is titrated with 12.00 mL of 5.00 x 10-3 M EDTA solution, what is the hardness of the water sample in ppm?
- 25.00 mL aliquots of the solution are titrated with EDTA to the Eriochrome Black T endpoint. A blank containing a small measured amount of Mg^{2+} requires 2.60 mL of the EDTA to reach the endpoint. An aliquot to which the same amount of Mg^{2+} is added
- The 25.00 mL sample of tap water required 12.82 mL of 0.0100 M solution of EDTA. Calculate the hardness
- In a titration experiment, 50.0 mL of 0.375 M HI solution is required to neutralize 35.0 mL of Ca(OH)_2 solution. What is the concentration of the Ca(OH)_2 solution? A) 0.134 M B) 0.536 M C) 34.2 M D) 0.268 M E) 68.5 M.
- Suppose 20.0 mL of a 0.750 M solution is diluted to 80.0 mL. Then 40.0 mL of this new solution is diluted to 250 mL. Finally, 25.0 mL of this solution is diluted to 175 mL. What is the concentration in moles per liter of the final solution?
- A solution of CaCl2 is prepared by dissolving 1.004 g of the solid in approximately 30 mL of water. How many moles of CaCl2 does this solution contain?
- A 25.0 mL solution of 0.0460 M EDTA was added to a 49.0 mL sample containing an unknown concentration of V^{3+} . All V^{3+} present formed a complex, leaving excess EDTA in solution. This solution was back-titrated with a 0.0490 M Ga^{3+} solution until
- A 50.0 mL sample containing Cd^2+ and Mn^2+ was treated with 68.8 mL of 0.0600 M EDTA. Titration of the excess unreacted EDTA required 12.7 mL of 0.0170 M Ca^2+. The Cd^2+ was displaced from EDTA by t
- Calculate the amount of , required to prepare 500 mL of 0.01 M EDTA solution.
- If you have a 5-mL sample of a 2.4 M solution of glucose, how many moles of the solute are present? If you place that 5 mL in a test tube with another 5 mL of deionized water, how many moles of the solute are present?
- How much of a 500 ml bottle of 1.00 molar KCI solution should be diluted with deionized water to give 200.0 ml of a 0.100 molar solution?
- Suppose 0.278 g of CaCl2 are dissolved into 1 L of distilled water. How many moles of Ca are in 50 mL of the 100 mg/L solution?
- A student analyzed powdered cultured buttermilk. A 2.270-gram sample of the powdered buttermilk required 37.18 mL of 1.183 x 10-2 M EDTA solution for titration of the Ca2+ ion. a. How many moles of Ca2+ ion were present in the sample? b. How many grams of
- 2. If 50 mL of 0.10 M HCI is diluted to a total volume of 100 mL by adding distilled water. what is the HCI concentration in the new solution? 3. How many moles of NaOH are required to neutralize al
- Suppose you dilute 20.0 mL of a 0.130 M solution of Na_2CO_3 to exactly 100.0 mL. You then take exactly 15.0 mL of this diluted solution and add it to a 250 mL volumetric flask. After filling the volu
- 25.0 mL tap water is titrated with 0.005 M EDTA. 7.95 mL EDTA is required for a complete reaction with water hardness. What is the molarity of the total water hardness?
- Mason J. O'Brien was given a 50.0 mL sample of a 0.56 M solution of HNO2. Using a buret, he transferred 25.0 mL of the weak acid into a 250 mL Erlenmeyer flask. He then titrated the acid with a standardized solution of 0.11 M NaOH. a. How many moles of th
- A 0.5 M solution, with a volume of 500 mL, is diluted to a volume of 1 liter. Calculate the number of moles of solute.
- A Sample of water has a hardness of 120ppm CaCO3. what is the concentration of ca2+ in moles/liter?
- A flask containing 5.00 mL of 3 M HCl solution requires 14.45 mL of 1.00 M NaOH for titration. How many moles of HCl are present in the solution? The density of 3 M HCl is 1.05 g / mL.
- A 25.0-mL solution of 0.0670 M EDTA was added to a 34.0-mL sample containing an unknown concentration of V3. All V3 present formed a complex, leaving excess EDTA in solution. This solution was back-titrated with a 0.0440 M Ga3 solution until all the EDTA
- d)If 50 mL of 0.2 M NaC2H3O2 and 10 mL of 1.0 M HC2H3O2 are diluted to a final volume of 100 mL, what is the molarity of NaC2H3O2 in the solution? e) If 50 mL of 0.2 M NaC2H3O2 and 10 mL of 1.0 M HC2
- How many millimoles of solute are present in 397 mL of a solution containing 7.86 ppm CaCO3?
- How many millimoles of solute are present in 533 mL of a solution containing 8.56 ppm CaCO3?