How many mL of a 0.160 M aqueous solution of copper(II) bromide, CuBr2, must be taken...

How many mL of a 0.160 M aqueous solution of copper(II) bromide, CuBr2, must be taken to obtain 5.86 grams of the salt? __ mL

Expert Solution

Molarity = number of moles of solute (1000) / volume of solvent in ml

Given, salt = 5.86 g ; molarity = 0.160 M

number of moles of solute = given mass /molar mass

Molar mass of Cu = 63.546 g and Br = 79.904 g

Molar mass of Copper(II) bromide; 63.546 +2(79.904) = 223.534 g/mol

Number of moles = 5.86g / 223.354 gmol^-1

= 0.0262

molarity = 0.0262 (1000) / vol. in ml

0.160 M = 0.0262 (1000) / vol. in ml

vol. in ml = moles (1000) / molarity

vol. in ml = 0.0262 (1000) / 0.160

vol. in ml = 26.2 /0.160

vol. in ml =163.75 ml

queen_honey_blossom answered 2 years ago

How many milliliters of an aqueous solution of 0.212 M copper(II) chloride is needed to obtain...

How many milliliters of an aqueous solution of 0.212 M copper(II) chloride is needed to obtain 6.74 grams of the salt?

You mix together 25.0 mL of a 0.025 M aqueous solution of copper(II) sulfate and 50.0...

You mix together 25.0 mL of a 0.025 M aqueous solution of copper(II) sulfate and 50.0 mL of 0.01 M sodium phosphate and isolate 68.3 mg of a precipitate. 1.Write the balanced equation for this reaction. Label all states. 2.What is the identity of the precipitate? 3.What is the theoretical yield of the reaction? 4.What is the percent yield of the reaction? You mix together aqueous solutions of 100.0 mL of 0.05 M sodium nitrate and 10.0 mL of potassium...

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM aqueous solution of potassium...

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) bromide is dissolved in it. Be sure your answer has the correct number of significant digits. The answer is needed in M. Thank you.

A 360.0 −mL buffer solution is 0.160 M in HF and 0.160 M in NaF. What...

A 360.0 −mL buffer solution is 0.160 M in HF and 0.160 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

35.12 mL of 0.263 M zinc bromide solution needs to react how many milliliters of with...

35.12 mL of 0.263 M zinc bromide solution needs to react how many milliliters of with 0.258 M cesium hydroxide solution?

how many grams of sodium bromide are there in 55.0mL of a 1.90M aqueous solution? please...

how many grams of sodium bromide are there in 55.0mL of a 1.90M aqueous solution? please answer as soon as possible and show work thank you

calculate how many mL of a 0.32 M solution of HCl must be added to an...

calculate how many mL of a 0.32 M solution of HCl must be added to an aqueous solution containing 4 g of Na2CO3 to obtain a solution at pH = 10. H2CO3 Ka1 = 4,5x10 -7 Ka2 = 4.8x 10 -10 A. 99,4 B. 80,8 C. 87,5 D. 33,9

1) The molar solubility of copper(II) sulfide in a 0.266 M copper(II) acetate solution is _______ M.

1) The molar solubility of copper(II) sulfide in a 0.266 M copper(II) acetate solution is _______ M. 2) The maximum amount of cobalt(II) carbonate that will dissolve in a 0.258 M cobalt(II) nitrate solution is _______ M.

An aqueous solution contains 0.419 M ammonia (NH3). How many mL of 0.305 M perchloric acid...

An aqueous solution contains 0.419 M ammonia (NH3). How many mL of 0.305 M perchloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.380. mL

An aqueous solution contains 0.459 M hydrocyanic acid. How many mL of 0.244 M potassium hydroxide...

An aqueous solution contains 0.459 M hydrocyanic acid. How many mL of 0.244 M potassium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.300? mL note in case u need this Acid/Base Ionization Constants at 25 oC Acid Formula Ka1 Ka2 Ka3 Acid/Base Ionization Constants at 25 oC Acid Formula Ka1 Ka2 Ka3 Acetic acid CH3COOH 1.8×10-5 Acetylsalicylic acid (aspirin) HC9H7O4 3.0×10-4 Aluminum ion Al(H2O)43+ 1.2×10-5...

Question