The pH of a lime is 1.90. What is the [H_3O^+]? A) 1.3 times 10^-2M H_3O^+...
What is the pH of a solution with [H_3O^+] = 1.0 times 10^-9 M?
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.
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
1x10ⓇM B 2x10 M 40 Normal gastric juice has a pH of about 2 and the gastric in is the concentration of HCl in the stomach? U10 M D 3x10 M of about 2 and the gastric juice is aqueous HCI. What 2 M HCI B 1.0x10' M HCI C 0.01 M HCI D 0.14 M HCI Ques. to, 41 Question What is the [H30'] of a sweat sample that has a pH = 5.8? A 2x10mm B3X10ⓇM 3x107M 42...
pH of urine is 5.7, while lime juice has a pH of 2.0. The urine sample has: a) approximately 100,000 times lower [H+] than the lime juice b) approximately 5,000 times lower [H+] than the lime juice c) approximately 3.5 times lower [H+] than the lime juice d) approximately 0.285 times the [H+] as the lime juice e) approximately 5 times lower [H+] than the lime juice
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 [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...
What is the conjugate base of H_2SeO_4 A) H_3O^+ B) HSeO_4^+ C) H_2SeO_4^- D) HS_eO_4^- E) H_3SeO_^+ In basic solution, ____. A) [OH^-] > 7.00 B) [H_3O^+] > [OH^-] C) [H_3O^+] < [OH^-] D) [H_3O^+] = [OH^-] E) [H_3O^+] = 0 M
What is pH when 0.2M acetic acid (Ka = 1.8 times 10^-5) is allowed to go to equilibrium. HAc + H_2O = = Ac^- + H_3O^+
The solubility products for Mg(OH)_2 and Ca(OH)_2 are 8.9 times 10^-12 and 1.3 times 10^-4, respectively Suppose a solution contains both Mg^2+ and Ca^2+ ions, each at 0.10 M in concentration (a) At what pH Mg(OH)_2 starts to from a precipitate? (b) At what pH Ca(OH)_2 begins to from a precipitate? (C) What is the concentration of Mg^2+ when Ca(OH)_2 begins to from precipitate?