7. An acid HA is dissolved in water: HA ---> H+ + A– . [HA] = 0.250 M ; [H+] = 4.00 x 10–4M ;
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[A–] = 4.00 x 10–4M. Calculate the pKa for the acid. Show your work below.
A monoprotic acid, HA, is dissolved in water: HA <------> H+ +A- The equilibrium concentrations of the reactants and products are [HA] = 0.280 M [H ] = 2.00 × 10–4 M [A–] = 2.00 × 10–4 M. Calculate the value of pKa for the acid HA.
A monoprotic acid, HA, is dissolved in water: HA- The equilibrium concentrations of the reactants and products are [HA] 0.100 M [H1- 2.00 x 104 M A1-2.00x10-4M Calculate the value of pKa for the acid HA. Number
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) – H(aq) + A (aq) The equilibrium concentrations of the reactants and products are [HA] = 0.270 M, [H+] = 4.00 x 10-4 M, and [A-] = 4.00 x 10-4 M. Calculate the value of pKa for the acid HA. pKa =
A monoprotic acid, HA, is dissolved in water: The equilibrium concentrations of the reactants and products are [HA] = 0.160 M [H ] = 4.00
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 1.33. This solution is titrated with a 0.250 M NaOH solution. 40.6 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What is...
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq)↽−−⇀H+(aq)+A−(aq) The equilibrium concentrations of the reactants and products are [HA]=0.280 M, [H+]=2.00×10−4 M, and [A−]=2.00×10−4 M. Calculate the value of pKa for the acid HA.
2.77 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 1.33. This solution is titrated with a 0.250 M NaOH solution. 44.2 mL of this NaOH solution is needed to reach the equivalence point. (a) (2 marks) What is the molar mass of HA? (b) (2 marks) What is the value of pKa for HA (aq)? (c) (2 marks) What is the pH at...
A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H2O(1) H2O+(aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.250 M, H,O+] = 2.00 x 10-4 M, and [A-] = 2.00 x 10-4 M. Calculate the Ka value for the acid HA. Ka = 6.79588
Question 12 of 13 > Hint Check Answe A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H2O(l) = H, 0+ (aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA) = 0.160 M, H, 0+) = 4.00 x 10--M, and A = 4.00 x 10-4 M. Calculate the K, value for the acid HA. K = 1
5 g of an unknown acid, HA, is dissolved in enough water to provide 25.0 mL of solution. The pH of this HA (aq) solution is 2.1 . This solution is titrated with a 0.210 M NaOH solution. 60.2 mL of this NaOH solution is needed to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the value of pKa for HA (aq)? (c) What is the pH at the equivalence point? (d) What...