The Kp of ethylamine is 4.30 x 104. What is the pH of a 0.08457M aqueous solution of ethylamine? CH3CH2NH2(aq) + (H2O() CH3CH2NH3*(aq) + OH (aq)

What is the net ionic reaction of HNO3 (a strong acid) with KOH (a strong base)? H2O (0)→ H+ (aq) + OH (aq) H+ (aq) + OH- (aq) → H₂O (1) HNO3(aq) + KOH (aq) → KNO3 (aq) + H₂O (1) K+ (aq) NO3(aq) →>> KNO3(aq)

HNO3(aq) is classified as a strong acid. The reaction equation with water would utilize which of the following arrows? Choice A Choice B 50% HNO3(aq) + H₂O(1) A NO3(aq) + H3O+ (aq) The approximate pH of the solution is >7 H₂S(aq) is classified as a weak acid. The reaction equation with water would utilize which of the following arrows? Choice A Choice B 50% H₂S(aq) + H₂O(1) BHS (aq) + H3O+ (aq) The approximate pH of the solution would be 4

A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) ⇒ H+ (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] A¯] = 3.00 × 10-4 M. Calculate the value of pK₁ for the acid HA. a pK₂: a = = 0.240 M, [H+] = 3.00 × 10−4 M, and

Butyric acid, CH3CH₂CH₂CH₂COOH, is a weak acid. It ionises in water to produce butanoate and hydronium ions. Select the correct balanced equation for the ionisation of butyric acid: Select one: a. CH3CH₂CH₂COOH → CH₂CH₂CH₂COO O b. CH3CH₂CH₂COO + H3O+ ⇒ CH³CH₂CH₂COOH + H₂O C. CH3CH₂CH₂COOH CH3CH₂CH₂COO¯ + H₂O+ O d. CH3CH₂CH₂COOH + H₂O ⇒ CH₂CH₂CH₂COO¯ + H₂O+

More H3O+ ions are added to an HCN and CN- buffer solution. Which reaction will occur to neutralize the additional H+ ions? H3O+ (aq) = HCN (aq) + H2O (1) HCN (aq) + H2O (l) = CN¯ (aq) + H3O+ (aq) H3O+ (aq) = CN¯ (aq) + H3O+ (aq) CN¯ (aq) + H3O+ (aq) = HCN (aq) + H₂O (1)

You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth.  Y2O + Y2O  ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths place

Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed.   ΔpH=?     Calculate the change in pH when 6.00 mL of 0.100 M NaOH is added to the original buffer solution.   ΔpH=?

Hippuric acid (HC3H&NO3), found in horse urine. Calculate the pH of a 0.250 M hippuric acid solution in water, if 0.155 M potassium hippurate salt, KC9H&NO3, was added. HC,H3NO3 (aq) + H20 (l) = H30*(aq) + C9H3NO3 *(aq) Ка = 2.40 x 10-4

Human blood has a pH of approximately 7.4 due to the carbonic acid/bicarbonate ion (H2CO3/HCO3−) buffer system. Any pH changes below 6.8 or above 7.8 can lead to death! Carbonic acid dissociates to form water and carbon dioxide in the equilibrium shown below. This process is crucial in respiration. H2CO3 (aq) ⇋ CO2 (g) + H2O pKa1 = 2.77 Carbonic acid dissociates in water to form the bicarbonate ion and the hydroxonium ion by the following equilibrium reaction:H2CO3 (aq) + H2O ⇋ H3O(aq)+ + HCO3− pKa2 = 3.70    (i) If there is a 25% increase in carbonic acid levels as per pKa1, explain how the body would deal with this change.