pKa

Some flowering plants will change color based on the pH of the soil.  For example, hydrangeas will flower in blue/purple shades under more acidic conditions and in pink/red shades under more basic conditions.  Consider NaHPO3 and NaHPO4.  Which compound, when added to soil, would be the better choice to cause hydrangeas to favor blue/purple shades?  Explain your reasoning.

Determine the quantity of sodium acetate (CHCOONa) needed to create buffer solution at a particular pH. Do this by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the mass of starting material required. The value of Ka for CH,COOH is 1.8 x 10°. Complete Parts 1-3 before submitting your answer. NEXT > Sodium acetate (CHCOONa) is added to an existing 500.0 mL solution of 0.200 M CH₂COOH to form a buffer with a pH equal to 5.000. Let x represent the concentration of CH,COO in the water after the addition of CH,COONa. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. CH,COOH(aq) Initial (M) Change (M) Equilibrium (M) + x 0.200 Н.О(1) 1.0 × 10 -1.0 × 10° 1.8 x 10° x x+1.0×10-x-1.0 10-18 10-x-18 10-1 -1.8 x 10 5.00 x + 5.00 -5.00 HO(aq) 1.0*10* + CH,COO (aq) RESET -1.0 x 10° x-5.00 x+ 10×10-x-1.0×10-* Determine the quantity of sodium acetate…

Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86.

Coral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer).       Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when    Ksp = 4.5 ´ 10–9.

2+ Given Ca²+ (aq) + CO3²−(aq) ⇒ CaCO3( s), Kc =2.2 × 10⁹. What is the value of the equilibrium constant for CaCO3(s) ≤ Ca²+ (aq) + 2- CO3²- (aq)? 2.2 × 108 4.5 × 10-⁹ -2.2 × 108 4.5 × 10⁹ 2.2 x 107 -8

When a 0.013 M aqueous solution of a certain acid is prepared, the acid is 0.73% dissociated. Calculate the acid dissociation constant K of the acid. Round your answer to 2 significant digits. x = 0 x10 X

1. State Le Chatelier’s Principle. If the equilibrium constant (K) ˃ 1, what will be the direction of the equilibrium position?                                                                                           [A/3]

The acid dissociation constant K of carbonic acid (H,CO, is 4.5 x 10'. a Calculate the pH of a 1.6 M solution of carbonic acid. Round your answer to 1 decimal place. pH