At 25 oC, Ammonia is a weak base that reacts with water according to this equation: ​NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq) Briefly explain how the equilibrium will shift (to get back to equilibrium) if the following perturbations are made to the system: (a) Addition of HCl
 (b) Addition of NaOH
 (c) Addition of NH4Cl

The ionization constant, Ka, for weak acid, HA, is 4.94 × 10–8.  What is the pH of a 0.7582 M solution of this acid? The equation for the ionization of weak acid HA as follows.             HA (aq) + H2O(l) ⇌ H3O+(aq) + A⁻(aq)

Write an equation for the ionizations of carbonic acid H2CO3 a weak acid write the equilibrium constant experession for this acid ionization

Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3).  (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

During a panic attack, a person hyperventilates (exhaling more CO2(g) than normal. Will this chemical equilibrium shift? If so, in what direction? Will the blood pH stay the same, increase, or decrease? Justify your reasoning and draw a concentration-time curve that represents this change.

Consider the following equilibrium. Would it lie more towards the reactants or the products? Why?  HCO3-(aq) + SO42-(aq) --> HSO4-(aq) + CO3-2(aq)

. (a) Calculate the pH of the following solution: 2.8 x 10-4 M Ba(OH)2 (b) What is the original molarity of a solution of HF whose pH is 1.7  at equilibrium?                           (Ka = 6.6 x 10-4)     HF (aq)  ⇌   H+ (aq) + F- (aq)

In the reaction NH3(aq) + H₂O(l) NH4+ (aq)+ OH(aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperature

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

Which of the following will increase the percentage of HF that is converted to the fluoride ion in water? (a) addition of NaOH (b) addition of HCl (c) addition of NaF