6) When the reversible reaction HC;H;O2 (aq) E→ H*(aq) + C¿H3O;'(aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of solid acetate (C;H;O;Na) to the reaction mixture? a) pH will not change because C;H;O;Na is not a part of the reaction equation. b) pH will not change because acetic acid and sodium acetate form a buffer c) pH will decrease because the reaction will shift towards reactants d) pH will increase because the reaction will shift towards reactants

A sample of solid sodium hydrogen phosphate is dissolved in water and allowed to come to equilibrium at 25 °C. NaH PO (aq) + H»O(1) = H2PO (aq) + NAOH(aq) 4 4 The OH concentration is measured and at equilibirum OH = 3.54 × 10 13 M. What is the pH of the solution? Type your answer...

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. ? NH3 (aq) + H20(1) NH4* (аq) + OH (аq) K =

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

For the Equilibrium Reaction: Na++ Cl-= NaCl  When adding Saturated NaCl+ 12 M HCl  What stress is applied? What is the direction of the shift?   When adding Saturated NaCl+ 3M HCl What is the stress applied? What direction is the shift?

URGENT!!! The equilibrium constant for the reaction between a weak acid and a weak base can be calculated from the relevant Ka, Kb and Kw using the rules for combining equilibrium constants. Find the Knet for the reaction between formic acid (HCO2H) and ammonia given the Ka (HCO2H) = 1.8 x 10⁻⁴ and Kb ammonia = 1.8 x 10⁻⁵.

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.

Calculate the pH of a 0.300 M NH4Cl solution. Kp for NH3 is 1.8 x 10-5.

Suppose you want to prepare a solution with a pH of 4.00 using acetic acid, CH3COOH, and sodium acetate, CH3CoOONa. What should the ratio of sodium acetate to acetic acid, CH3CO0-| : [CH3COOH], be in your buffer solution? Hint: The Ka for acetic acid is 1.8x105. 0.18:1 O 1.9:1 0.84:1 O 5.5:1 O 1:1

Calculate the pH for each case in the titration of 50.0 mL of 0.110 M HClO(aq)0.110 M HClO(aq) with 0.110 M KOH(aq).0.110 M KOH(aq). pka = 7.40 ka= 4.0*10^-8 What is the pH after addition of 50.0 mL KOH? What is the pH after addition of 60.0 mL KOH?