# Calculate the concentration (M) of copper in each sample. The Cu^2 standard solution was prepared...

## Question:

Calculate the concentration (M) of copper in each sample. The {eq}\displaystyle \rm Cu^2 {/eq} standard solution was prepared by dissolving {eq}\displaystyle \rm 3.928 \ g \ CuSO_4 \cdot 5H_2O {/eq} into {eq}\displaystyle \rm 1.000 \ L {/eq} distilled water.

The {eq}\displaystyle \rm NH_4OH {/eq} used in these solutions is {eq}\displaystyle \rm 3 \ M {/eq}. Following are the mixtures for the solutions:

Solution {eq}\displaystyle \rm 1: 7.50 \ mL {/eq} standard {eq}\displaystyle \rm Cu^{2+}: 0.00 \ mL, \ H_2O: 2.50 \ mL \ NH_4OH {/eq}

Solution {eq}\displaystyle \rm 2: 6.00 \ mL {/eq} standard {eq}\displaystyle \rm Cu^{2+}: 1.50 \ mL \ H_2O: \ 2.50 \ mL \ NH_4O {/eq}

## Volume:

Volume is one factor on which the molarity of a solution depends. If the volume of a solution is either increased/decreased by adding/removing the solvent, then the molarity of a solution changes.

## Answer and Explanation: 1

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

View this answerThe amount of {eq}\rm CuSO_4.5H_2O {/eq} in its standard solution is 3.928 g.

The molar mass of {eq}\rm CuSO_4.5H_2O {/eq} is 159.6 g/mol

The...

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 2Learn about the mole ratio. Understand the definition of mole ratio, how to find mole ratio in stoichiometry, and see examples of using mole ratio in problems.

#### Related to this Question

- Calculate the concentration of 12.5 g of copper (II) sulphate dissolved to form 30M of solution.
- Calculate the concentration (molarity) of copper(ii) sulfate, CuSO_4, in 1L of a solution containing 200 g Copper-Sulfate-Pentahydrate (CuSO_4 \cdot 5H_2O)?
- Consider the following : Weigh out 1.25 g of CuSO4 X 5H2O and add it to 40 mL of distilled water. Mix well until the copper sulfate is in solution. Add distilled water until 50 mL of solution. This is solution A. Calculate the concentration of soluti
- Calculate the mass (in g) of CuSO_4 \cdot 5H_2O (MM = 249.68 g/mol) necessary to prepare 50.0 mL of a solution having a concentration of 0.500 M CuSO_4.
- The final volume of the solution is 284 mL. What is the concentration of CuSO_4 in the final solution, in mol/L? mass = 1.787 g of CuSO_4 \cdot 5H_2O = 7.157 times 10^{-3}
- A solution contains 37 g CuSO4 and 111 g of water. Calculate the concentration by mass of solution.
- Calculate the molar concentration of a solution prepared by dissolving 80.0 g of CuSO_4 \cdot 5H_2O insufficient water to obtain 1500 L of solution.
- What is the % concentration (m/v) of a solution prepared by dissolving 160.0 g of CuSO_4 in enough water to make 250 mL of a solution?
- If you add 4.00 mL of pure water to 6.00 mL of 0.0250 M CuSO_4, what is the concentration of copper (II) sulfate in the diluted solution?
- Calculate the actual concentration of Cu2+ ion in your samples. Because you are simply diluting a copper-containing solution of known concentration, you can use the equation: (conc. of original soluti
- A 0.25 M CuSO_4 solution is required. A student is given 60 g of copper sulphate. Calculate the volume of water needed to dissolve copper sulphate crystals and make this solution.
- What is the concentration of a solution formed by diluting 7 ml of 5.4M CuSO_4 \cdot 5H_2O solution to 50ml?
- In an experiment designed to determine the concentration of Cu^{+2} ions in an unknown solution, you need to prepare 100 mL of 0.10 M CuSO_4 as your stock solution. How many grams of CuSO_4 (s) should
- In the laboratory you dissolve 17.7 g of copper (II) 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 copper (II) cation? c. What is the concentration of
- Calculate the mass of Copper (II) sulfate CuSO_4 needed to make 3.00 L of 3.0 M solution?
- Calculate the mass of copper(II) sulfate pentahydrate needed to prepare 0.600 M stock solution of copper (II) from solid copper (II) sulfate pentahydrate, CuSO_4 cdot 5H_2O.
- What is the total molar concentration of the ions in a 0.0150 M CuSO4 solution in water?
- What is the total molar concentration of all the ions in a 0.0300 M CuSO4 solution in water?
- Determine the concentration of copper ion in solution, you desire to make 0.2 M copper(ii) solution. how many grams of C u S O 4 5 H 2 O (fw is 249.69 g?mol) are required to make 25.00 ml of this solution?
- Calculate the mass percent of CuSO_4 in a solution whose density is 1.30 g/mL and whose molarity is 1.36 M. %CuSO_4 =
- Calculate the mass (in grams) of CuSO4 you must measure out to prepare 100 mL of a 0.025 M CuSO4 solution.
- calculate the molarity of each ion in a 0.025 aqueous solution of (a) kcl; (b) CuSO4; (c) CaCl2
- If 4.00 mL of 0.0443 M CuSO4 is diluted to 10.0 mL with pure water, what is the molar concentration of copper(II) sulfate in the diluted solution?
- A 65.25 g sample of CuSO_4.5 H_2O (M= 249.7) is dissolved in water to make 0.800 L of solution. What volume of this solution must be diluted with water to make 1.00 L of 0.100 M CuSO_4?
- If you have a solution of copper sulfate and water with a molarity of 0.5, a volume of 0.5 L, and 0.25 moles of copper sulfate, what will the concentration (molarity) be if the solution is diluted to 1 L of water?
- Calculate the volume of 1.0 M CuSO_4 stock solution you should use to make 100 mL of a 0.010 M CuSO_4 solution.
- Prepare 20 mL of 0.050 M CuSO4 solution by mixing 1 mL of 1.0 M CuSO4 solution with 19 mL of distilled water. Setup a concentration cell in two wells of the cell you made by adding 5mL of 0.050 M CuSO
- A chemist must prepare 725 mL of 275 mM aqueous copper(II) sulfate (CuSO4) working solution. He'll do this by pouring out some 0.316 M aqueous copper(II) sulfate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the
- If 2.40 g of CuSO4 is dissolved in 8.57 x 10^2 mL of 0.360 M NH3, calculate the concentrations of Cu^2+, NH3, and Cu(NH3)4^2+.
- Determine the molarity of each of the following solutions. (a) 2.78 kg of CuSO4 7 H2O in 315 L of solution (b) 0.005531 mol of Cl2 in 10.40 mL of solution (c) 0.000890 g of C2H5NO2 in 2.20 mL of solution
- You have prepared a solution by diluting 12.00 mL of 0.790 M copper (II) nitrate to a total volume of 50.00 mL. What is the concentration of Cu^{2+} ions in the resulting solution? Give your answer to
- Determine the mass of CuSO_4 . 5 H_2O that is needed to prepare 50.00 mL of a 0.07000 M solution.
- If you mix 3.0 mL of CuSO4 (0.060 M) with 12.0 mL of HNO3 (1.0 M), how do you calculate the concentration of CuSO4?
- Calculate the mass of solid required to prepare 100 mL of a .50 M aqueous solution copper II sulfate pentahydrate.
- In the laboratory, you dissolve 20.7 g of copper(II) fluoride 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 concentration of
- Consider the following steps below: Weigh out 1.35 g of CuSO_4 \times 5H_2O and add to 35 mL of distilled water. Mix well until the copper sulfate is in solution. Add distilled water until there is 55 mL of solution. This is solution A. Calculate the c
- If 2.0 mL of 0.80M copper (II) sulfate and 8.0 mL of water are mixed, what is the concentration of the resulting solution?
- Calculate the mass of CuSO_4.5H_2O required to prepare 50 mL of 0.040 M CuSO_4 solution.
- A chemist prepares a solution of copper(II) sulfate (CuSO_4) by measuring out 14.5 mu mol of copper(II) sulfate info a 200 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's copper(II)
- What is the total molar concentration of all the ions in 0.040 M solutions of the following salts in water? (a) 0.040 M KCl. (b) 0.040 M CuSO_4. (c) 0.040 M CaCl_2.
- Calculate the volume needed to dissolve 11.2 g CuSO_4 to prepare 0.140 M?
- Determine how much CuSO4-5H2O is required to prepare a 50ml solution of 0.0200M CuSO4
- You are given two solutions. Solution A is made by dissolving 4.0 g of copper sulfate in 100 mL water. Solution B is made by dissolving 5.0 g of copper sulfate in 150 mL water. Which has the higher concentration, or are they the same?
- Determine the molarity of a solution containing 2.5 moles CuSO_4 in 4.2 L of water.
- How could you prepare 250 mL of a 0.35 M CuSO4 solution from a 2.00 M CuSO4 solution?
- How could you prepare 300 mL of a 0.25 M CuSO4 solution from a 2.00 M CuSO4 solution?
- How would you prepare 150 mL of a 0.800% (w/v) CuSO4 solution from a 0.182 M CuSO4 solution?
- The molarity of the copper solution in the cuvet below was determined by spectrometric analysis to be 2.90 times 10^{-2} M Cu. Calculate the grams of copper in the Jefferson nickel used to make the initial solution.
- To make 800mL of a 0.25 M solution of CuSo_4 how much 1M CuSo_4 solution would be needed?
- How would you prepare 10 mL of 0.5 mL CuSO_4 cdot 5H_2O solution from 10 M CuSO_4 cdot 5H_2O?
- If 25.00 mL of 5.80 M CuSO_4 solution is diluted to 2.0 L, what is the molarity of the diluted solution?
- How many mL of a 1.10 M CuSO4 solution must be diluted to make 602 mL of a 0.400 M CuSO4 solution?
- An aqueous solution is 15.0% by mass of copper(II) sulfate pentahydrate, CuSO_4 . 5H_2O. What is the molarity of CuSO_4 in this solution at 20 degrees C? The density of this solution at 20 degrees C is 1.167 g/mL.
- Find the mass percent of CuSO_4 in a solution whose density is 1.30 g/mL and whose molarity is 1.36 M.
- Can you explain how to prepare 150 mL of a 0.800% (w/v) aqueous CuSO4 solution using a 0.182 M CuSO4 stock solution?
- A chemist has a supply of CuSO_4 solution that contains 230 gram per liter of water. She wishes to make a copper sulphate solution that has a solution of 200.0 grams per liter how much of her copper sulphate solution should she use and how much water shou
- What is the molarity of a solution that contains 23.095 g of CuSO4 in 103.9 mL of solution?
- What is the molar concentration of 65.5 g of copper (i) sulfate dissolved in 2.4 L of H2O?
- In a lab, 67.2 g of copper (II) chloride is dissolved in enough water to make 250 mL of solution. What is the molar concentration of the solution? a. 2.5 mol/L b. 2.0 mol/L c. 1.0 mol/L d. 0.50 mol/L
- What is the molarity of a solution prepared by dissolving 160.0 g of CuSO_4 in enough water to make 250 mL of a solution?
- A 0.1025 g sample of copper metal is dissolved in 35 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 200 mL. Calculate the molarity of Cu2+ in the solution.
- Calculate the concentration, in moles per liter, of a fertilizer solution, if 500.0 ml of the solution contains 1.84 g of copper sulphate, CuSO_4.
- A chemist must dilute 72.5 mL of 341 mM aqueous copper(II) sulfate (CuSO4) solution until the concentration falls to 97.0 mM. How much distilled water should be added to the solution? What is the final volume?
- Explain how you would make 10.00 mL of a 0.03 M Cu^{2+} solution from a standard solution of 0.10 M CuSO_4.
- If you dissolve 0.135 g of copper in nitric acid and dilute it to 100.0 mL with water, calculate the concentration of Cu^{2+} in the resulting solution.
- Determine the concentration of Cl- in a 0.30 M CuCl2 solution.
- How many grams of CuSO_4 cdot 5H_2O are needed to prepare 50 ml of a 0.75 M solution?
- What is the mass of CuSO4 needed to prepare a 125 mL solution of 3.5 M?
- Calculate the molarity of 71 g of CuSO4 5H2O in 8.2 L of solution.
- 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
- Molarity, is the concentration of a solution expressed in terms of moles solute per liter of solution. What is the molarity of a solution that contains 27.250 g CuSO_4 in 181.8 mL?
- If you dissolve 0.135 grams of copper in nitric acid and dilute it to 100.0 mL with water, how would you calculate the concentration of Cu+2 in the resulting solution? Show step by step calculations.
- What is the molarity, expressed in mol/L, of a solution composed of 3.76 g of copper nitrate in 110.7 mL of water? Express your answer to three decimal places. The molar mass of copper nitrate is 187.5558 g/mol.
- Calculate the volume of 1.747 M copper (II) nitrate that must be diluted with water to prepare 225.8 mL of a 0.6180 M solution.
- A chemist must dilute 89.5 mL of 5.48 mM aqueous copper (II) fluoride CuF_2 solution until the concentration falls to 4.00 mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in
- How would you prepare a 500 ml solution of 5% CuSO4 using CuSO4.5H2O hydrate?
- What is the total molarity of all the ions present in 0.1 M CUSO_4 and 0.1 M Al_2(SO_4)_3 solution?
- A solution was made by adding 0.291 grams of copper (II) thiocyanate to a 500 mL volumetric flask and diluting to the mark. Determine the concentrations in the solution: A) ppm copper (II) thiocyanate AND ppm copper (II) ion B) ppm thicyanate ion AND pp
- A 0.1052 g sample of copper metal is dissolved in 55 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 208.5 mL. Calculate the molarity of Cu2+.
- What is the molarity in mol/L of a solution composed of 2.21 g of copper nitrate in 97.2 mL of water? The molar mass of copper nitrate is 187.5558 g/mol.
- Calculate the mass of copper (ii) sulphate which needs to be used to prepare 500 cm^3 of a 0.1 M solution.
- What is the molarity of a solution with a volume of 974 mL containing 17 g of CuSO4?
- Within the concept of "drinking water standards", what is the molarity of the copper atoms or ions in a drinking water sample, that has a concentration of copper just equal to the indicated MCLs (maximum contamination levels) allowed for copper in drinkin
- In the laboratory, you dissolve 13.6 g of copper(II) nitrate 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 concentratio
- 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 mass of CuSO_4 times 5H_2O is required to prepare 4.0 mL of 0.040 M CuSO_4 solution?
- 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
- Describe how you could prepare 105 mL of a 0.32 M CuSO4 5H2O solution.
- Describe how you could make 10 mL of a 0.5 M CuSO4 5H2O solution from a 10.0 M CuSO4 5H2O solution.
- How many grams of CuSO4 5H2O are needed to prepare 150.0 mL of a 0.75 M CuSO4 solution?
- Calculate the number of moles of CuSO_4 contained in 100 ml of 1mole CuSO_4 solution. Also, find the number of SO_4^{2-} ions in it .?
- (a) Give the equation for Beer's Law and identify the 4 variables in the equation. (b) A stock solution of copper sulfate has a concentration of 1.00 M. Calculate the concentration of a solution ma
- a) How do you make 100.00 mL of 0.1000 M copper (II) sulfate solution? b) From your prior solution, how would you prepare 25.00 mL for each of 0.0800 M, 0.0600 M, 0.0400 M, 0.0200 M and 0.0080 M copper (II) sulfate?
- How will you prepare 0.33% solution of CuSO4 (solid) of 400ml? From 0.33% CuSO4, show the preparation of 0.11% CuSO4 of 150 ml.
- A 0.1052 g sample of copper metal is dissolved in 55 mL of concentrated HNO_3 to form Cu^{2+} ions and then water is added to make a total volume of 208.5 mL. Calculate the molarity of Cu^{2+}.
- A 4.7% (m/v) CuSO4 solution has a volume of 57.4 mL. How many grams of CuSO4 are in the sample? a. 0.082 g b. 8.2 g c. 820 g d. 0.27 g e. 2.70 g
- Calculate the following quantity: Volume of 2.238 M copper (II) nitrate that must be diluted with water to prepare 438.6 mL of a 0.6227 M solution.
- Calculate the molarity (M) for each of these solutions: (a) 31.45 g of NaCl in 1.50 L (b) 14.41 g of MgS in 0.750 L (c) 0.4567 g of CuSO_4 in 825 mL (d) 25.5 mg of NaCN in 5.00 mL
- Suppose that 2.25 grams of CuSO4 are dissolved in 930 mL of 0.30 M ammonia. What concentration (Molarity) of Cu2+ ion is expected to be free in the aqueous solution and not bound to ammonia in the com
- Calculate the number of milliliters of 0.10 M cupric sulfate solution that must be diluted to prepare 10 mL of a 0.015 M cupric sulfate solution.