You have been asked to do a dilution of a copper sulfate solution. The solution to be diluted is...
Question:
You have been asked to do a dilution of a copper sulfate solution. The solution to be diluted is {eq}2.88 \ M {/eq} copper sulfate. What volume of the {eq}2.88 \ M {/eq} copper sulfate is required to make {eq}250 \ mL {/eq} of {eq}1.03 \ M {/eq} copper sulfate solution?
Dilution
A solution's concentration can be changed by increasing or decreasing the quantity of a solute or a solvent. When the quantity of the solvent is increased, it is termed as dilution.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer
Given data:
- The concentration of stock solution of copper sulfate {eq}\left( {{M_1}} \right){/eq} is 2.88 M.
- The concentration of diluted solution...
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
Calculating Dilution of Solutions
from
Chapter 8 / Lesson 5
101K
Want to know how to calculate dilution factor? See dilution equations, the dilution formula, and learn how to dilute acid and how to dilute a solution.
Related to this Question
- What volume of the 1.5 M copper sulfate is required to make 250 mL of 1.03 M copper sulfate solution?
- What mass of solid copper (II) sulfate is needed to make 500.0 ml of .0300 M copper (II) sulfate 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?
- How much copper sulfate is needed to make a solution of 100ml of 1M copper sulfate?
- 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?
- 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.
- 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?
- 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?
- How many mL of a 5.0 M copper(II) sulfate solution must be added to 150 mL of water to achieve a 0.25 M copper(II) sulfate solution?
- When you made your solution of Copper (III) sulfate, why did you only add 80-90 % of the water, dissolve the solid and then raise the volume to the target of 100 ml?
- 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?
- What volume of water should be added to 500 mL of a 1.0 mol/L CuSO_4 solution to dilute it to 0.5 mol/L?
- How many mL of a 1.10 M CuSO4 solution must be diluted to make 602 mL of a 0.400 M CuSO4 solution?
- 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.
- How many grams of Copper (II) sulfate pentahydrate would you use to make 400.0 mL of 0.750 M solution?
- Weight of anhydrous copper (II) sulfate would be required to make one liter of a solution containing 10.0 g of Cu^{2+} ions per liter what height of copper (II) sulfate pentahydrate would be required to make the solution.
- What volume of 0.120 M CuSO_4 is required to give 0.150 mol of copper(II) sulfate, CuSO_4?
- An experiment calls for 100 mL of 0.1 M copper (II) sulfate solution. Write a step-by-step procedure for a science teacher to make 100 mL of 5 M stock solution and the required diluted solution.
- 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?
- How many mL of copper (II) stock solution are required to make 25.00 mL of a 0.181 M solution?
- To what volume should you dilute 121 mL of an 7.90 M CuCl_2 solution so that 52.0 mL of the diluted solution contains 4.81 g CuCl_2?
- To what volume should you dilute 126 mL of an 8.10 M CuCl_2 solution so that 50.5 mL of the diluted solution contains 4.52 g CuCl_2?
- To what volume should you dilute 130 ml of an 8.40 m CuCl_2 solution so that 65.0 ml of the diluted solution contains 5.9 g CuCl_2?
- To what volume should you dilute 126 ml of a 7.90 M CuCl_2 solution so that 49.5 ml of the diluted solution contains 5.9 g CuCl2?
- To what volume should you dilute 150 mL of an 8.00 M CuCl2 solution so that 55.0 mL of the diluted solution contains 5.9 g of CuCl2?
- To what volume should you dilute 132 mL of an 8.00 M CuCl2 solution so that 52.0 mL of the diluted solution contains 4.33 g of CuCl2?
- What volume should you dilute 124 mL of an 8.10 M CuCl_2 solution so that 52.0 mL of the diluted solution contains 5.9 g CuCl_2 ?
- 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)?
- Cu(NO_3)_2 \cdot 3H_2O (FW 241.58) will be used to prepare your copper stock solution. How much will you need to make up 250 mL of stock solution containing 250 \mu g/mL (= 250 ppm) as copper (250ppm Cu)?
- What volume of 0.120M cuso4 is required to give 0.150 mol of copper2 sulfate, cuso4?
- 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?
- Calculate the concentration of 12.5 g of copper (II) sulphate dissolved to form 30M of solution.
- What volume of water would be required to dilute a 10.0 mL 0.650 M solution of calcium sulfate to create 0.25 M solution, what would the volume of the new solution be?
- Calculate the volume in milliliters of a 0.65 M copper(II) sulfate solution that contains 100 grams of copper(II) sulfate.
- 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?
- To what volume should you dilute 127 mL of a 7.95 M CuCl2 solution so that 49.5 mL of the diluted solution contains 4.77 g of CuCl2?
- To what volume should you dilute 128 mL of an 8.05 M CuCl2 solution so that 51.0 mL of the diluted solution contains 4.43 g CuCl2?
- To what volume should you dilute 132 mL of a 7.95 M CuCl2 solution so that 48.5 mL of the diluted solution contains 4.75 g CuCl2?
- 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
- If the absorbance of a solution of copper ion decreases by 45% upon dilution, how much water was added to 15.0 mL of a 1.00 M solution of Cu_{2} +?
- 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?
- How many mL of 5% BaCl2.2H20 solution was required to precipitate sodium sulfate. what if the sodium sulfate was potassium sulfate instead. Would the volume requirement be higher or lower than the sodium sulfate and why?
- What volume of water should be added to 200 mL of 0.100 M aluminum sulfate to prepare a solution with 0.050 M of sulfate ion?
- How many mL of 0.109 M Na2CO3 would be needed to precipitate all of the copper ions in 26.7 mL of 0.159 M CuSO4?
- Calculate the mass of solid required to prepare 100 mL of a .50 M aqueous solution copper II sulfate pentahydrate.
- What is the molarity of a solution with a volume of 974 mL containing 17 g of CuSO4?
- What is the molar concentration of 65.5 g of copper (i) sulfate dissolved in 2.4 L of H2O?
- 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
- Assuming the sample is pure sodium sulfate, how many mL of 5% BaCl_2.2H_2O solution would be required to precipitate the sulfate. Density of barium shloride solution of 1.00 g/mL.
- What mass of copper(ii) sulphate (GFM = 159.5) is required to make 400 cm^3 of 0.5 mol/L solution?
- 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 student prepares a 2M solution of copper sulfate. She adds 17 mL of the solution to a 100 mL volumetric flask and dilutes it up to a final volume of 100 mL with water. What is the final molar concen
- If the absorbance of a solution of copper (II) ion decreased by 33.0 percentage upon dilution, what volume of water was added to 20.0 mL of a 1.20 M solution of Cu^{2+} (aq)?
- 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?
- 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.
- What is the concentration of a solution formed by diluting 7 ml of 5.4M CuSO_4 \cdot 5H_2O solution to 50ml?
- If 30 mL of 0.299 M sodium hydroxide solution is added to a 50.0 mL of a 0.950 M solution of copper sulfate solution, what mass in grams (g) of the precipitate will form?
- What volume (in mL) of a 0.250 M sodium sulfate solution is needed to precipitate all the barium, as barium sulfate, from 12.5 mL of a 0.150 M barium nitrate solution?
- A solution of copper(II) sulfate is prepared by placing 5.80 g copper(II) sulfate in a flask and adding enough water to prepare 125 mL of solution. When 25.0 mL sample of the solution is added to 125 mL of sodium hydroxide (0.125 M), determine the mass of
- You need to make an aqueous solution of 0.219 M cobalt(II) sulfate for an experiment using a 300 mL volumetric flask. How much solid cobalt(lI) sulfate should you add?
- What is the mass of CuSO4 needed to prepare a 125 mL solution of 3.5 M?
- 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
- 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.
- 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
- 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.
- You need to make an aqueous solution of 0.196 M Iron(III) sulfate for an experiment in the lab, using a 500 mL volumetric flask. How much solid Iron(III) sulfate should you add?
- A). To what volume should you dilute 121 mL of an 8.00 M CuCl2 solution so that 52.0 mL of the diluted solution contains 4.44 g CuCl2? B). Silver nitrate solutions are often used to plate silver onto
- Calculate the concentration (M) of copper in each sample. The Cu^2 standard solution was prepared by dissolving 3.928 g CuSO_4 cdot 5H_2O into 1.000 L distilled water. The NH_4OH used in these solutions is 3 M. Following are the mixtures for the solution
- 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}
- How many grams of solute are required to make a 558 ml solution of copper (ii) chloride with a concentration of 2.3497 M?
- If you dilute 1 mL of 0.5 M aluminum sulfate up to 1 L, what is the molarity of the diluted solution?
- If you dilute 1 mL of aluminum sulfate up to 1 L, what is the molarity of the diluted solution?
- How many grams of CuSO4 do you need to make 500 mL of a 0.10 M solution?
- How many grams of CuSO4 do you need to make 400 mL of a 0.15 M solution?
- If the absorbance of a solution of copper(II) ion decreases by 16.00% upon dilution, what volume of water was added to 20.0 mL of a 1.20 M solution of Cu^2+(aq)?
- Calculate the volume needed to dissolve 11.2 g CuSO_4 to prepare 0.140 M?
- Determine the volume of water (in mL) that was added to 29.9 mL of the stock solution (2.94M) to prepare a 0.855 M copper (II) perchlorate solution.
- 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
- What is the molarity of a solution that contains 23.095 g of CuSO4 in 103.9 mL of solution?
- Determine the sulfate ion concentration in a solution prepared by diluting 15.00 mL of a 0.200 M aluminum sulfate solution with 35.00 mL of water. Assume the volumes are additive.
- What mass of CuSO_4 times 5H_2O is required to prepare 4.0 mL of 0.040 M CuSO_4 solution?
- 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.
- You need to make 4200 mL of 0.450 M CuSO4. How many grams of CuSO4 do you need?
- What volume of 0.10 M CuSO_4 will completely dissolve 1.0 g Zn?
- 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
- 1. Assume that you start with 0.495 g of copper turnings: a)Calculate the initial number of moles of Cu. b) Calculate the minimum volume of 16.0 M HNO₃ required to dissolve all of the copper (
- Some solid copper(II) sulfate is dissolved in sufficient water to make 100.0 mL of solution. Enough of a sodium hydroxide solution of concentration 0.1500 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?
- What weight of anhydrous copper (II) sulfate would be required to make one liter of a solution containing 10.0 g of Cu^{2+} ions per liter?
- 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 =
- Can 1750 mL of water dissolve 4.6 moles of copper sulfate (CuSO4)? Explain why or why not.
- How do you prepare approximately 100 ml of a 0.12 M copper (II) chloride solution using a 50.5% by mass copper (II) chloride that has a density of 1.05 g/ml?
- How many grams of CuCl_2 are required to make 75 ml of a 0.20 M solution?
- How many mL of 0.122 M Na2CO3 would be needed to precipitate all of the copper ions in 23.7 mL of 0.167 M CuSO4? How many grams of CuCO3 could be recovered?
- Determine the mass of CuSO_4 . 5 H_2O that is needed to prepare 50.00 mL of a 0.07000 M solution.
- How many grams of CuSO_4 cdot 5H_2O are needed to prepare 50 ml of a 0.75 M solution?
- 3. If you added 0.832 g of Mg to a solution containing 1.794 g of CuSO_4, to reduce any copper ions present, what is the least volume of 6.0 M HC1 you would need to dissolve the excess Mg? Explain why
- How many mL of 0.0250 M CuSO4 solution contains 1.75 g of solute?
- Can 1750 mL of water dissolve 4.6 moles of copper sulfate? Why or why not?
- To make 800mL of a 0.25 M solution of CuSo_4 how much 1M CuSo_4 solution would be needed?
Explore our homework questions and answers library
Browse
by subject