[GE-CHM 101] Acids and Bases

An aqueous solution of HNO3 has a pH of 2.34. What is the concentration of the acid?

• 2.18 x 10^(-12) M

• 0.0046 M

• 2.34 M

• 11.66 M

What is the pH of a 0.0011 M solution of Ca(OH)2?

• 0.0011

• 2.66

• 10.84

• 11.34

What is the concentration of a solution of Ca(OH)2 for

which the pH is 11.68?

• 1.1 x 10^(-12) M

• 2.1 x 10^(-12) M

• 2.4 x 10^(-3) M

• 4.8 x 10^(-3) M

• 1.5 x 10^(-5)

• 1.5 x 10^(5)

• 6.7 x 10^(-10)

• 6.7 x 10^(10)

A 0.020 M solution of niacin has a pH of 3.26. Calculate the percent ionization of the niacin.

• 1.4%

• 1.6%

• 2.7%

• 5.4%

What is the pH of a 0.010 M solution of niacin? The pKa of niacin is 1.5 x 10^(-5).

• 2.00

• 3.41

• 4.82

• 6.82

What is the pH of a buffer solution that is 0.45 M acetic acid (HC2H3O2) and 0.85 M sodium acetate (NaC2H3O2)? The Ka for acetic acid is 1.8 × 10–5.

• 0.071

• 4.74

• 5.02

• 5.30

The titration of 25.00 mL of an HCl solution of unknown concentration requires 26.54 mL of a 0.100 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution?

• 0.0265 M

• 0.053 M

• 0.106 M

• 0.212 M

Tags

NGSS.HS-PS1-7