Calculate the [NH₃] in a solution of 0.330 M ammonium fluoride (NH₄F). Hint: Use the Ka of HF (6.8 × 10⁻⁴) and the Kb of NH₃ (1.8 × 10⁻⁵) to calculate Kc for the reaction NH₄⁺(aq) + F⁻(aq) ⇌ NH₃(aq) + HF(aq).

What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka.  You will need the value of Ka.  Look it up on the chart (p 4 of packet) Solve for x Find the pH           The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…

3. Dihydrogen phosphate anion, H₂PO4¹, is an amphoteric species. Write two chemical equations that show the amphoteric properties of dihydrogen phosphate anion. Label each entity on the reactant and the product side as acid or base. Determine the equilibrium constants. H₂PO4 (aq) + H₂0 (1) H₂PO4 (aq) + H₂0 (1) K= K=

The strongest known acid is fluoroantimonic acid, [H₂F][SbF6]. It is 1016 times more acidic than concentrated sulfuric acid and has a pH of -31.3; it is strong enough to protonate both xenon and molecular hydrogen. It is an ionic liquid made by reacting hydrogen fluoride with antimony(V) fluoride: 2 HF + SbF5 → H₂F+ + SbF6 Explain why this acid is so strong.

Calculate the [NH₃] in a solution of 0.250 M ammonium fluoride (NH₄F). Hint: Use the Ka of HF (6.8 × 10⁻⁴) and the Kb of NH₃ (1.8 × 10⁻⁵) to calculate Kc for the reaction NH₄⁺(aq) + F⁻(aq) ⇌ NH₃(aq) + HF(aq). Want solution ASAP Your answer

Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M HCl(aq) solution. Calculate the pH at 10.0 mL intervals of added HCl(aq), up to 50.0 mL, and plot the titration curve. Assume that the volumes are additive. Use pKb = 3.34 for methylamine.

Calculate the pH of a solution that is 3.67×10−53.67×10-5 M NH3 and 2.41×10−52.41×10-5 M NH4Cl.Kb=1.821.82 x 10−510-5NH4+1 (aq) + H2O(l) <----> NH3(aq) + H3O+1(aq)

We want to prepare a buffered solution having a pH of 4.97 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONA). Ką for formic acid is 1.8 x 10-4. Incorrect. Calculate the ratio [HCOO (aq)] / [HCOOH(aq)] in the buffered solution required to achieve a pH of 4.97. [HCOO (aq)] /[HCOOH(aq)] = i 1.68E1 eTextbook and Media Hint Save for Later Attempts: 2 of 3 used Submit Answer

H2C2O4 is a diprotic acid that dissociates as shown below.Ka1 = 5.38 x 10-2 and Ka2 = 5.18 x 10-5. Determine the pH of 0.1 M Sodium hydrogen oxalate (NaHC2O4). (Note: neglect hydroxide formation due to hydrogen oxalate  hydrolysis)

Calculate the [NH₃] in a solution of 0.480 M ammonium cyanide (NH₄CN). Hint: Use the Ka of HCN (4.9 × 10⁻¹⁰) and the Kb of NH₃ (1.8 × 10⁻⁵) to calculate Kc for the reaction NH₄⁺(aq) + CN⁻(aq) ⇌ NH₃(aq) + HCN(aq).