chemistry

A chemist dissolves 0.097 g of CuSO4 · 5 H2O
in water and dilutes the solution to the mark
in a 500-mL volumetric flask. A 13.6-mL
sample of this solution is then transferred to a
second 500-mL volumetric flask and diluted.
What is the molarity of CuSO4 in the second
solution?
To prepare the second 500 mL of solution
directly, what mass of CuSO4 · 5 H2O would
need to be weighed out?
Answer in units of mg

  1. 👍
  2. 👎
  3. 👁
  1. First, calculate the M of the initial solution.
    mols CuSO4.5H2O = grams/molar mass = ?
    Then mols/L = M

    So the diluted solution is M of first x (13.6/500) = ?

    For the last part.
    How many mols do you have in the second solution? That's mols = M x L = ?
    Then mols = grams/molar msss. You know molar mass and mols, solve for grams.

    1. 👍
    2. 👎
  2. y=mx+b

    1. 👍
    2. 👎
  3. -b+or- square root of b^2 -4ac/2a

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    A chemist dissolves 0.096 g of CuSO4 · 5 H2O in water and dilutes the solution to the mark in a 500-mL volumetric flask. A 10.8-mL sample of this solution is then transferred to a second 500-mL volumetric flask and diluted. What

  2. chemistry

    The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 13.9 g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0°C to

  3. Chemistry

    Calculate the volume of 1.0 M CuSO4 stock solution you should use to make 100 mL of a 0.010 m CuSO4 solution.

  4. Chem 11

    So I did a lab determining the chemical formula of a hydrate. I really just need somebody to check this over for me. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks

  1. Chemistry

    Magnesium sulfate is often used it first aid hot-packs giving off heat when dissolved in water. When 2.00 g of MgSO4 dissolves in 15.0 mL of water (d= 1.00g/mL) at 25.0ºC, 1.51 kJ of heat is evolved. A) Write the balanced

  2. Chemistry!!

    A chemist wants to prepare a stock solution of H2SO4 so that a sample of 20.00mL will produce a solution with a concentration of .50 M when added to 100.0mL of water. A)what should the molarity of the stock solution be? B)If the

  3. Chemistry

    A)How many moles of O2 are required for the complete combustion of 2.2 g of C3H8 to form CO2 and H2O? b)A 65.25 g sample of CuSO4•5H2O (M = 249.7) is dissolved in enough water to make 0.800 L of solution. What volume of this

  4. Chemistry

    2) To the solution in problem 1 (d) at 100 degrees celsius, 10g of water are added, and the solution is cooled to 0 degrees celsius... (problem 1d: the number of grams of water required to dissolve a mixture containing 15 g KNO3

  1. chem

    Calculate the number of moles required to make 100 mL of a 3.0 M solution of CuSO4·5 H2O. is the answer .03? if not walk me through the steps thanks

  2. chemistry

    Consider the following reaction. SO3(g) + H2O(l) → H2SO4(aq) A chemist allows 60.9 g of SO3 and 11.1 g of H2O to react. When the reaction is finished, the chemist collects 54.4 g of H2SO4. Determine the limiting reactant,

  3. Chemistry

    DR.BOB 22 PLS HELP A chemist dissolves 0.099 g of CuSO4 · 5 H2O in water and dilutes the solution to the mark in a 500-mL volumetric flask. A 28.9-mL sample of this solution is then transferred to a second 500-mL volumetric flask

  4. Chemistry

    Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)→H2SO4(aq) A chemist allows 61.5 g of SO3 and 11.2 g of H2O to react. When the reaction is finished, the chemist collects 51.0 g of H2SO4. Determine

You can view more similar questions or ask a new question.