Calculate the molar concentrations of H+ and OH– in solutions that have the following pOH values. Enter values in scientific notation, for example 0.0010 would be 1.0E-3.
a) 7.29
[OH-]:
[H+]:
b) 1.66
[OH-]:
[H+]:
c) 10.86
[OH-]:
[H+]:
d) 13.47
[OH-]:
[H+]:
e) 5.98
[OH-]:
[H+]:
Calculate the molar concentrations of H+ and OH– in solutions that have the following pOH values....
Calculate the molar concentrations of H+ and OH– in solutions that have the following pOH values. Enter values in scientific notation, for example 0.0010 would be 1.0E-3. a)7.18 b)1.93 c)10.64 d)13.21 e)5.45
I can't figure these questions out. Help would be appreciated! Calculate the molar concentrations of H+ and OH in solutions that have the following pOH values. Enter values in scientific notation, for example 0.0010 would be 1.0E-3. x Incorrect. Did you remember to include the negative signs in the pH and pOH equations? a) 12.07 [OH): 71.4E-13 6.9E-2 [H+]: Correct. b) 7.00 [OH-]: 1.0E-7 [H+]: 1.0E-7 3.1.0-7 SHOW SOLUTION x Incorrect. Did you remember to include the negative signs in...
calculate the molar concentration of OH- in water solutions with the following H3O molar concentrations: October 29, 2017 at 5:18 PM H. Calculate the molar concentration of OH in water solutions with the following H,0 molar concentrations: . a 1.0 x 107 • b. 4.7 X 10-11 . c. 1.2 . d. 0.043
9.29 Calculate the molar concentration of H3O+ in water solutions with the following OH- molar concentrations: a) 1.0 x 10^-5 b) 3.4 x 10^-4 c) 8.3 x 10^-9 d) 0.072 e) 3.2
Calculate the molar concentration of OH^- in water solutions with the following H_3O^+ molar concentrations. [H_3 O^+] = 0.068 M [OH^-] = __________ M [H_3 O^+] = 5.8 times 10^-4 M [OH^-] = _________ M [H_3 O^+] = 0.0068 M [OH^-] = ____________ M [H_3 O^+] = 6.0 times 10^-10 M [OH^-] = __________ M [H_3 O^+] = 6.0 times 10^-2 M [OH^-] = _____________ M
Calculate the [H^+], [OH^-], pH and pOH of the following solutions: a. 0.01 M HCl (aq) b. 0.02 M NaOH (aq)
Calculate the [OH]-, the pH and the pOH for each of the following solutions AND identify each of the solutions as acidic, basic, or neutral. a. [H+] = 1.0 x 10-7 b. [H+] = 7.4 x 10-16 c. [H+] = 10 M d. [H+] = 6.3 x 10-4 Show work please
15.32. Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. a. [OH-] = 7.69 X 10 M b. [OH-] = 2.18 x 10-'M c. [H-] = 4.0 x 10-8 M d. [H+] = 3.56 X 10-4 M
Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. Complete parts 1-4 below. Part 1: [OH–] = 9.31×10-3M A: pH B: pOH Choose one: Acidic,Basic,Neutral Part 2: [OH–] = 5.49×10-9M A: pH B: pOH Choose one: Acidic,Basic,Neutral Part 3: [H+] = 4.93×10-8M A: pH B: pOH Choose one: Acidic,Basic,Neutral Part 4: [H+] = 4.15×10-4M A: pH B: pOH Choose one: Acidic,Basic,Neutral
Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...