For the following reactions, predict which direction the reaction will shift with the addition of hydrochloric acid. Cu2+ (aq) + 4Cl- (aq) [CuCl4]2- (aq) CaCO3(s)+H+(aq)Ca2+(aq)+HCO3-(aq)

Predict which of these acid-base reactions are product-favored and which are reactant-favored. In each case write a balanced equation for any reaction that might occur, even if the reaction is reactant-favored. Consult Table 14.2 if necessary. H2O(ℓ) + HNO3(aq) H3PO4(aq) + H2O(ℓ) CN−(aq) + HCl(aq)

Write the equilibrium constant expression for this reaction: 2H* (aq) + CO²(aq) → H₂CO3(aq) Olo

Write the equilibrium constant expression for this reaction: CH;Cl(aq)+OH (aq) → CH;OH(aq)+Cl (aq)

Write the equilibrium constant expression for this reaction: H;PO,(aq) - 3 H (aq)+PO (aq) ?

A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.

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The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)

Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants.  If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35   HCOOH(aq) ↔ HCOO–(aq) + H+(aq)        Ka = 1.80 × 10-4   i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places

Write the equilibrium constant expression for this reaction: →>> H3PO4(aq) 3 H(aq) +PO(aq)