Analytical Chemistry: Solutions

If 73.5 mL of 0.200 M KI was required to precipitate all of the lead (II) ion from an aqueous solution of lead(II) nitrate, how many moles of Pb²⁺ were originally in the solution?

• 7.25 × 10^-3 moles of Pb²⁺

• 7.35 × 10^-3 moles of Pb²⁺

• 7.55 × 10^-3 moles of Pb²⁺

• 7.45 × 10^-3 moles of Pb²⁺

• None of the above

Tags

NGSS.HS-PS1-7

One method of determining the concentration of hydrogen peroxide (H2O2) in a solution is through titration with the iodide ion. The net ionic equation for this reaction is

A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12 mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in the sample?

• 0.1114 M

• 0.4041 M

• 0.1010 M

• 0.2227 M

• 5.568 × 10^-2 M

Tags

NGSS.HS-PS1-7

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M?

• 12.4 g

• 8.8 g

• 3.11 g

• 6.21 g

• 24.9 g

Tags

NGSS.HS-PS1-7

The concentration of oxalate ion (C₂O₄^2-) in a sample can be determined by titration with a solution of permanganate ion (MnO₄^-) of known concentration. The net ionic equation for this reaction is

A 30.00 mL sample of an oxalate solution is found to react completely with 21.93 mL of a 0.1725 M solution of MnO₄^-. What is the oxalate ion concentration in the sample?

• 0.4312 M

• 0.05044 M

• 0.3152 M

• 0.02914 M

• 0.1821 M

Tags

NGSS.HS-PS1-7

Which of the following is the equivalent of 4.3 ppm sodium ion concentration?

• None of the above

• 430 ppb

• 0.043 ppb

• 4300 ppb

• 0.0043 ppb

34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H₂SO₄ solution. What is the concentration of the original sulfuric acid solution?

• 0.209 M

• 0.105 M

• 0.0229 M

• 0.218 M

• 0.0523 M

Tags

NGSS.HS-PS1-7

A 110. mL solution of 0.340 M HCl(aq) is mixed with a solution of 330. mL of 0.150 M HNO₃(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H⁺ are present in the final solution?

• 0.490 moles H⁺

• 0.0435 moles H⁺

• 0.0869 moles H⁺

• 0.415 moles H⁺

• 0.374 moles H⁺

Tags

NGSS.HS-PS1-7

1.40 g of silver nitrate is dissolved in 125 mL of water. To this solution 5.00 mL of 1.50M hydrochloric acid is added, and a precipitate form. Find the concentration of silver ions remaining in solution.

• 5.7 × 10^-3 M

• 5.9 × 10^-3 M

• 0.121 M

• 6.34 × 10^–2 M

• 5.77 × 10^–2 M

Tags

NGSS.HS-PS1-7

Which one of the following would be immiscible with water?

• A

• B

• C

• D

• E

Tags

NGSS.HS-ESS2-5

What mass of Li3PO4 is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

• 3.38 g

• 30.4 g

• 19.3 g

• 6.75 g

• 10.1 g

Tags

NGSS.HS-PS1-7