A 1.0-L buffer solution contains 0.300 mol acid, HA, and 0.300 mol base, NaA. The value of K, for the acid HA is 2.9x10-8. Ignoring the small volume change, what is the most likely pH of the solution if a 10.0 mL- sample of 1.00M HNO3 is added to the original buffer? 11.30 < pH < 11.45 O 7.45 < pH < 7.60 O 6.34 < pH < 6.49 く O 3.65 < pH < 3.78 く

An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M solution of HIO,. The p K, of ammonia is 4.74. Calculate 3' the pH of the base solution after the chemist has added 99.0 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places.

A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H­O­-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation

What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride? K, (methylamine) = 4.4 × 10-4

what is the pH of a buffer solution containing 0.100 M acetic and 0.050 M sodium acetate. The Ka for acetic acid is  1.82×10^-5:

Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc). Ka for HAc is1.8x10 -5.  How much NaOH must be added to reach the equivalence point, and what is the pH at the equivalence point?

A buffer solution is 0.400 M in HF and 0.349 M in KF. If Ka for HF is 7.2 × 10-4, what is the pH of this buffer solution? pH = ||

propionic acid, ?a=1.34×10−5,Ka=1.34×10−5, 3.00 M sodium propionate, CH3CH2COONa   1. The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? ( in g) 2. Based on this information, what volume of acid should the student measure to make the buffer solution? (in ml)

13

25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka of acetic acid is 1.8x10-5. What is the pH of the solution after adding NaOH?