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Chapter 4: Problem 41

Describe how you would prepare 2.00 L of each of the following solutions. a. 0.250 M NaOH from solid NaOH b. 0.250 M NaOH from 1.00 M NaOH stock solution c. 0.100\(M \mathrm{K}_{2} \mathrm{CrO}_{4}\) from solid $\mathrm{K}_{2} \mathrm{CrO}_{4}$ d. 0.100\(M \mathrm{K}_{2} \mathrm{CrO}_{4}\) from 1.75 $\mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}$ stock solution

Short Answer

Expert verified
a. Dissolve 20.00 g of solid NaOH in water and dilute to a final volume of 2.00 L in a volumetric flask. b. Measure 0.500 L of the 1.00 M NaOH stock solution and dilute it to a final volume of 2.00 L in a volumetric flask. c. Dissolve 38.84 g of solid K2CrO4 in water and dilute to a final volume of 2.00 L in a volumetric flask. d. Measure 0.114 L of the 1.75 M K2CrO4 stock solution and dilute it to a final volume of 2.00 L in a volumetric flask.

Step by step solution

01

Calculate moles of NaOH

For a 2.00 L solution and a 0.250 M concentration, we will Calculate moles of NaOH using the given formula: \(moles = M \times V\) moles of NaOH = \((0.250 M) \times (2.00 L) = 0.500\) moles
02

Calculate the mass of NaOH

The molar mass of NaOH is 40.00 g/mol. To find the mass of NaOH needed: mass of NaOH = \((0.500\, moles) \times (40.00\, g/mol) = 20.00 g\)
03

Prepare the solution

Dissolve 20.00 g of solid NaOH in water and dilute to a final volume of 2.00 L in a volumetric flask. b. 0.250 M NaOH from 1.00 M NaOH stock solution
04

Calculate moles of NaOH

Same as in part a, we have 0.500 moles of NaOH.
05

Calculate the volume of stock solution

Using the stock solution concentration to find the volume needed: volume of stock solution = \(\frac{0.500\, moles}{1.00 M} = 0.500 L\)
06

Prepare the solution

Measure 0.500 L of the 1.00 M NaOH stock solution and dilute it to a final volume of 2.00 L in a volumetric flask. c. 0.100 M K2CrO4 from solid K2CrO4
07

Calculate moles of K2CrO4

For a 2.00 L solution and a 0.100 M concentration: moles of K2CrO4 = \((0.100 M) \times (2.00 L) = 0.200\) moles
08

Calculate the mass of K2CrO4

The molar mass of K2CrO4 is 194.19 g/mol. To find the mass of K2CrO4 needed: mass of K2CrO4 = \((0.200\, moles) \times (194.19\, g/mol) = 38.84 g\)
09

Prepare the solution

Dissolve 38.84 g of solid K2CrO4 in water and dilute to a final volume of 2.00 L in a volumetric flask. d. 0.100 M K2CrO4 from 1.75 M K2CrO4 stock solution
10

Calculate moles of K2CrO4

Same as in part c, we have 0.200 moles of K2CrO4.
11

Calculate the volume of stock solution

Using the stock solution concentration to find the volume needed: volume of stock solution = \(\frac{0.200\, moles}{1.75 M} = 0.114 L\)
12

Prepare the solution

Measure 0.114 L of the 1.75 M K2CrO4 stock solution and dilute it to a final volume of 2.00 L in a volumetric flask.

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Most popular questions from this chapter

What volume of 0.100\(M \mathrm{NaOH}\) is required to precipitate all of the nickel(Il) ions from 150.0 \(\mathrm{mL}\) of a \(0.249-M\) solution of \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2} ?\)

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide

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