A solution contains 0.352 M HA (Ka = 4.66⋅10−64.66⋅10-6) and 0.758 M NaA.
What is the pH of this solution? | |
What is the pH of this solution after 0.138 mol of HCl are added to 1.00 L of this solution? | |
What is the pH of this solution after 0.276 mol of HCl are added to 1.00 L of this solution? |
A solution contains 0.352 M HA (Ka = 4.66⋅10−64.66⋅10-6) and 0.758 M NaA. What is the...
A 1.00 L solution contains 0.352 M HA (Ka = 4.66⋅10−64.66⋅10-6) and 0.758 M NaA. What is the pH of this solution? What is the pH if 0.310 L of 0.138 M KOH is added to the solution be? What is the pH if 0.620 L of 0.138 M KOH is added to the solution be?
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.
A solution contains 0.250 MHA(Ka-1.0 x 106and 0.45 M NaA. What is the pH after 0.30 mole of HCl is added to 1.00 L of this solution? a. 7.44 .2.10 98.56 8.5.44 e.0.52
A 1.00 L solution contains 0.311 M HA (K3 = 3.04 - 10 ) and 0.796 M NaA. What is the pH of this solution? What is the pH if 0.318 L of 0.158 M KOH is added to the solution be? What is the pH if 0.636 L of 0.158 M KOH is added to the solution be?
A 1.00 L solution contains 0.326 M HA (Kg = 5.09 · 10-7. and 0.796 M NaA. What is the pH of this solution? What is the pH if 0.325 L of 0.219 M KOH is added to the solution be? What is the pH if 0.650 L of 0.219 M KOH is added to the solution be?
A solution contains 0.250 M HA (К.-1.0 added to 1.00 L of this solution? 3. 10" and 0.45 M NaA. what is the pH after 0.30 mole of HC1 is a. 0.52 b. 7.44 c. 5.44 d. 2.10 e. 8.56
What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66*10^-7. pH = __________ What is the \rm pH after 0.150 mol of \rm HCl is added to the buffer from Part A? Assume no volumechange on the addition of the acid. pH = _____________ What is the \rm pH after 0.195 mol of \rm NaOH...
Question 1 : HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M. Question 2 : We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA. Question 3 : We place 0.661 mol of a weak acid, HA,...
Part A What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Express the pH numerically to three decimal places. pH = SubmitHintsMy AnswersGive UpReview Part Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid....
100 mL of buffer solution that is 0.15M HA (Ka= 6.8x10-5) and 0.20M NaA is mixed with 29.7mL of 0.25M HCl. What is the pH of the resulting solution?