[H3O+] = 1.0*10-9M
pH = -log[H3O+] = -log(1.0*10-9)
= -log1.0 + 9log10
= 0 + 9
pH = 9.0 (E)
What solution is considered basic? [H_3O^+] = 1.0 times 10^-7 [H_3O^+] = 1.0 times 10^-4 [OH^-] = 1.0 times 10^-7 [H_3O^+] = 1.0 times 10^-10
The pH of a lime is 1.90. What is the [H_3O^+]? A) 1.3 times 10^-2M H_3O^+ B) 7.9 times 10^-13M H_3O^+ C) 1.3 times 10^12M H_3O^+ D) 1.9 M H_3O^+ E) 7.9 times 10^1 M H_3O
Calculate the pH of each solution. [H_3O^+] = 6.2 times 10^-6 M Express your answer using two decimal places. pH = 5.21 [H_3O^+] = 6.4 times 10^-4 M Express your answer using two decimal place t.
Calculate the [OH^-] of each aqueous solution with the following [H_3O^+] a. vinegar, 1.0 times 10^-3 M b. urine, 5.0 times 10^-6 M c. ammonia, 1.8 times 10^-12 M d. NaOH, 4.0 times 10^-13 M
Calculate the pH of an aqueous solution containing 1.0 times 10^-2 M HCl, 1.0 times 10^-2 M H_2SO_4, and 1.0 times 10^-2 M HCN.
Calculate the [H_3O^+] and pH of the following polyprotic acid solution 0.340 M H_2C_2O_4. Calculate the pH of this solution
Hint Calculate the pH of exh solution at 25 ℃- 1.0×10-4 M Ha pH= 1.0×10-4 M NaOH pH= 001 M KOH pH = 0 Arrange the aqueous solutioms from the most acidic to the mst basic, at 25'C Acidic Basic Answer Blandk F12 8 9 0 :: Expand 411% Resources Hint 23 Classify each apanous solution aode, basic, or neuthl at 25C Acidic Basic Neutral 9 0
calculte pH
.1.0 x 10-9 M solution of HNO3.
What is the pH of a 1.0 M Na_2CO_3(aq)? Ka of HCO_3 = 4.7 times 10^-11 Equation:
Calculate the [H_3O^+] for the following conditions a. pH = 3.21 b. pOH= 13.34 Calculate the pH of the following solutions: a. 3.7 times 10^-3 M HCl b. 8.6 times 10^-2 M HC_2H_3O_2 K_a = 1.74 times 10^-5 Calculate the pH of the following buffer a. 7.8 times 10^-2 M HC_2H_3O_2 and 8.6 times 10^-2 M NaC_2H_3O_2 A buffer is made from 3.7 times 10^-1 M HC_2H_3O_2 and 2.9 times 10^-1 M NaC_2H_3O_2 a. What is the pH? B. If...