Which of the following compounds could be used to create a buffer with a pH of 9.00? ammonia, Kb = 1.76 x 10–5 None of the above compounds could be used to create a buffer with a pH of 9.00. p-toluidine, pKb = 8.92 formic acid, Ka = 1.80 x 10–4 benzene-1,2,3-tricarboxylic acid, pKa1=2.88, pKa276, pKa3 = 7.13

A buffer solution is prepared which is 0.260 M both in lactic acid (CH3CHOHCO2H) and in sodium lactate (CH3CHOHCO2Na). Ka = 1.38×10-4 for lactic acid. What is the pH of this solution? When 1.42 mL of 0.140 M HCl is added to 14.0 mL of this buffer solution, what is resulting change in pH?

help with the following question ( use kg for the mass)

11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?

An analytical chemist is titrating 198.6 mL of a 0.7200M solution of formic acid (H₂CO₂) with a 0.7700M solution of KOH. The p K of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 209.6 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

1. The ionization constant (Kb) of pyridine (C5H5N) is 5.62 x 10–4. If 11.3 grams of sample of pyridine is dissolved in 250.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in mineral absorption. A 0.125 M solution of this acid is found to have a pH of 2.034. Based on the table below, what most likely is the identity of this unknown acid? (Note: For this problem, treat the acid as if it is a monoprotic acid.)

Consider an acetate buffer, initially at the same pH as its pka (4.76). When sodium hydroxide (NaOH) is mixed with this buffer, the O pH rises more than if the same amount of NaOH is added to an acetate buffer initially at pH 6.76. pH remains constant. ratio of acetic acid to acetate ion in the buffer decreases. sodium acetate formed precipitates because it is less soluble than acetic acid. pH rises more than if the same amount of NaOH is added to unbuffered water at pH 4.76.

A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C₆H₅NH₃⁺ in the solution. The value of Kb for C₆H₅NH₂ is 3.8 × 10⁻¹⁰. Let x equal the original concentration of C₆H₅NH₃⁺ in the water. Based on the values given, set up an ice table to determine the unknown. Based on the ice table, set up the expression of Kb in order to determine the unknown. Do not simplify or combine terms. Based on the ice table and kb expression, determine the original concentration of C₆H₅NH₃⁺.

An analytical chemist is titrating 165.5 mL of a 1.100 M solution of propionic acid (HC,H,CO,) with a 0.3900 M solution of KOH. The p K of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 497.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ?

Given the Kb's of three weak bases and the Ka's of two weak acids choose the one that could be used as one of the components of a buffer solution with a pH of 6.35. 1. CH3COOH (Ka = 1.8 x 10–5) 2. NH2OH (Kb = 1.1 x 10–8) 3. CH3NH2 (Kb = 4.4 x 10–4)   4. C5H5N (Kb = 1.7 x 10–9) 5. HCOOH (Ka = 1.8 x 10–4)