Enough of a monoprotic weak acid is dissolved in water to produce a 0.01 10 M solution. The pH of the resulting solution is 2.62. Calculate the K₂ for the acid. K₁ = X10 TOOLS

explain why the ph doesnt change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the base NH3 and a salt of its conjugate acid NH4CL

If the K, of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.42 M solution of this acid? pH =

Consider the following reaction at equilibrium. CH,COOH(aq) = CHyco0 (aq) + H*(aq) When NaCH3CO0 is added to the solution will the value of the equilibrium constant, K, and the pH of the solution increase, decrease, or remain the same? Select one: O A. K, decreases and pH increases O B. Ka remains the same and pH decreases O C. Ka decreases and pH remains the same O D. K, remains the same and pH increases O E. K, increases and pH decreases

3.

A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 0.01534 L sample of her gastric juices and titrate the sample with 0.000185 M KOH. The gastric juice sample required 0.00645 L of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration.

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0110 M solution. The pH of the resulting solution is 2.62. Calculate the K₂ for the acid. K₂= Ka

8.) A solution is made where 0.878 moles HCl is added to water that has a total volume of solution of 1855mL. What is the pH of the solution. НС(аq) — н' (аq) + CГ(aq)

If a buffer solution is 0.250 M in a weak acid (?a=5.9×10−5) and 0.450 M in its conjugate base, what is the pH?

Hypobromous acid, HBrO, can be produced commercially as a disinfectant. A solution is made by dissolving 3.73 kg of pure HBrO in distilled water to make 10.0 L of solution. A pH pribe determines that the pH of the aqueous solution is 3.98.  What is the value of Ka for HBrO?