write a balanced equilibrium equation showing the dissociation and b) write the equilibrium constant expression and c) give the Ka value

(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.

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…

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. CSHSNHI 04- D2+ 3+ 4+ 1 2 4 5 7 9 3 Os (s) (1) (g) (aq) + OH- NR H H3O+ C H2O Reset • x H2O Delete CO LO

$ Which of the following statements comectly describes the b solution? O In bases JOH is greater than 1 On bases, (OH) is less than HO In acids OH is greater than 01 O in bases, (OH) 14,0 In neutral solutions [H0] MO D Question 6 According to LeChâtelier's principle, predict whether adding the direction of reactants, products, or no change Nhà loại + HỌC NH + HO O reactants O no change O products p

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5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.

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

Acid-Base Equilibrium: 1. Find the pH of 0.0500M CH;CICOOH (a weak acid) where Ka=1.4 x 103 2. Ca(OH); is a strong base (meaning that nearly 100% ionizes). Find the pH for 5.0 x 103 M solution of Ca(OH)2.