Calwlate the ph of the solution [H+] = lo 1 x 10-3M [1++] = 6.0 x10-"M

Question

Question

science chemistry

Answer 1

Answer #1

pn = -log [n+7.11 pn == log ſlo137073M] pn = 2.95 1 pn= -log ent] the-log [ 6.0x10=m] pn = 10.22

Answer 2

Similar Homework Help Questions

Calculate H,0*] for a 5.32 x 10-M HBr solution. H,0+1 = x10 Calculate (H,0+) for a...

Calculate H,0*] for a 5.32 x 10-M HBr solution. H,0+1 = x10 Calculate (H,0+) for a 1.50x 10 ? M KOH solution. [H,0+) = X10 x10
Calculate the [H+] and pH of a 1.23 x 10-4 M nitrous acid solution. The K,...

Calculate the [H+] and pH of a 1.23 x 10-4 M nitrous acid solution. The K, of nitrous acid is 7.10 x 10-5. [H+] = 1.4 X10-4 pH = 3.9
Calculate the pH of a solution if the concentration of H+ is 5.8 x10^(-6) M (1...

Calculate the pH of a solution if the concentration of H+ is 5.8 x10^(-6) M (1 point O 14 O 2.54 0 5.24

Calculate the (OH) and the pH of a solution with an (H+] = 3.2 x 10-"...

Calculate the (OH) and the pH of a solution with an (H+] = 3.2 x 10-" Mat 25 °C. [OH-] = pH = Calculate the (H+) and the pH of a solution with an (OH) = 7.0 x 10 M at 25 °C. M [H*] pH Calculate the (H+) and the [OH-] of a solution with a pH = 8.56 at 25 °C. M M (он) Calculate either [H2O+] or [OH-] for each of the solutions. Solution A: [OH-] =...
The acid dissociation K, of propionic acid (C,H,CO,H) is 1.3 x 10 Calculate the pH of a 3.0 x10 Maqueous solution o...

The acid dissociation K, of propionic acid (C,H,CO,H) is 1.3 x 10 Calculate the pH of a 3.0 x10 Maqueous solution of propionic acid. Round your answer to 2 decimal places. x 5 ?
Calculate the [OH-] and the pH of a solution with an (H+] = 1.2 x 10-1°...

Calculate the [OH-] and the pH of a solution with an (H+] = 1.2 x 10-1° Mat 25 °C. [OH-] = M pH = Calculate the [H+) and the pH of a solution with an [OH-] = 7.2 x 10-11 M at 25 °C. M pH = Calculate the (H+) and the [OH-] of a solution with a pH = 1.31 at 25 °C. M [**] M [OH"] = Calculate the hydroxide ion concentration, [OH-], for a solution with a...

= 6.0 x 10- For the diprotic weak acid HỌA, K.1 = 2.6 x 10- and...

= 6.0 x 10- For the diprotic weak acid HỌA, K.1 = 2.6 x 10- and K What is the pH of a 0.0650 M solution of HLA? pH = What are the equilibrium concentrations of H, A and A- in this solution? [HA] =
Q6.1 2 Points What is the pH of the following solution? [H'] = 1.25x10-3M pH =...

Q6.1 2 Points What is the pH of the following solution? [H'] = 1.25x10-3M pH = Enter your answer here Q6.2 2 Points What is the pH of the following solution? [H'] = 5.67x10-8 M pH = Enter your answer here Q6.3 6 Points You have a solution with pH 4.17. What is the TH3O+ =
Calculate the pH of a solution that is 1.50 M in HCN (Ka = 6.2 x10-10)...

Calculate the pH of a solution that is 1.50 M in HCN (Ka = 6.2 x10-10) and 0.50 M in NaCN. A. 3.44 B. 8.73 C. 9.68 D. 9.21 E. 3.63

6.What is the pH of a solution with [OH-] = 1.7 x 10-3M? 7.Calculate [H3O+] of...

6.What is the pH of a solution with [OH-] = 1.7 x 10-3M? 7.Calculate [H3O+] of a solution with a pH of 5.5 8. A 15.0 mL sample of H2SO4solution is titrated with 24.0 mL of 0.245 M NaOH solution. What is the molarity of the H2SO4solution?H2SO4(aq) + 2 NaOH (aq) →2 H2O (l) + Na2SO4(aq)