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Exam 13: Aqueous Equilibria

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Question 31

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A buffer contains equal concentrations of a weak acid,HA,and its conjugate base,A^-.If the value of K_a for HA is 1.0 * 10^-9,what is the pH of the buffer?

A) 13.0
B) 5.0
C) 7.0
D) 1.0
E) 9.0

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Question 32

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You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,phenol (pK_a = 9.89) ,aniline (pK_b = 9.37) ,HNO₂ (pK_a = 3.37) ,CH₃NH₂ (pK_b = 3.44) .Which two reagents would you use to make a buffer with a pH of 10.5?

A) HCl and CH₃NH₂
B) HCl and aniline
C) NaOH and phenol
D) NaOH and HNO₂
E) HCl and phenol

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Question 33

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What is the main factor that determines the pH of any buffer?

The K_sp for mercury(I) iodide is 1.2 * 10^-28.What is the solubility of mercury(I) iodide?

The following compounds are available as 0.10 M aqueous solutions. Pick two solutions that could be used to prepare a buffer with a pH of ~ 4.

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.20 M KOH(aq).This solution is a buffer.

Consider the titration of 15.0 mL of 0.200 M H₃PO₄(aq) with 0.200 M NaOH(aq) .What is/are the major species in solution after the addition of 30.0 mL of base?

Which of the following indicators would be most suitable for the titration of 0.10 M (CH₃) ₃N(aq) with 0.10 M HClO₄(aq) ? For trimethyamine,pK_b = 4.19.

What is the equilibrium constant for the titration reaction involving HClO₄(aq) and Ba(OH) ₂(aq) ?

If equal volumes of 0.004 M Pb(NO₃) ₂(aq) and 0.004 M KI(aq) are mixed,what reaction,if any,occurs? The value of K_sp for PbI₂ is 1.4 * 10^-8.

What is the equilibrium constant for the reaction HCN(aq) + OH^-(aq) →CN^-(aq) + H₂O(l)

A buffer solution contains 0.25 M NaNO₂(aq) and 0.80 M HNO₂(aq) (pK_a = 3.37) .What is the pH after 0.10 mol HBr are added to 1.00 L of this buffer?

You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,HCN (pK_a = 9.31) ,aniline (pK_b = 9.13) ,HNO₂ (pK_a = 3.25) ,and CH₃NH₂ (pK_b = 3.34) .Which two reagents would you use to make a buffer with a pH of 10.6?

How many moles of KOH(s)must be added to 1.00 L of 0.782 M HF(aq)to produce a buffer with a pH = 4.00?

The curve for the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq)is given below.What are the main species in the solution after 7.5 mL of base have been added?

A buffer solution contains 0.75 mol KH₂PO₄ and 0.75 mol K₂HPO₄.What is the pH after 0.10 mol KOH is added to 1.00 L of this buffer? The pK_a of H₂PO₄^- is 7.21.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq) ,the final concentrations of HClO(aq) and ClO^-(aq) ,respectively,are

A buffer solution contains 0.0200 M acetic acid and 0.0200 M sodium acetate.What is the pH after 2.0 mmol of NaOH are added to 1.00 L of this buffer? pK_a = 4.75 for acetic acid.

What is the equilibrium constant for the titration reaction involving CH₃NH₂(aq) and HBr(aq) ?

What is the pH of an aqueous solution that is 0.10 M HCOOH (K_a =1.8 * 10^-4) and 0.10 M NaHCO₂?