Question

In: Chemistry

What are [HCOOH], [H3O+], [HCOO–], [OH–] and pH of a) 0.300 M HCOOH, b) 0.005 M...

What are [HCOOH], [H3O+], [HCOO–], [OH–] and pH of

a) 0.300 M HCOOH,

b) 0.005 M HCOOH solutions? (Ka = 1.8·10–4)

HCOOH(aq) + H2O(l) H3O+(aq) + HCOO–(aq)

Expert Solution

HCOOH(aq) + H2O(l)--------------> H3O+(aq) + HCOO–(aq)

I 0.3 0 0

C -x +x +x

E 0.3-x +x +x

Ka = [H3O^+][HCOO^-]/[HCOOH]

1.8*10^-4 = x*x/0.3-x

1.8*10^-4 *(0.3-x) = x^2

x= 0.00726

[HCOOH] = 0.3-x = 0.3-0.00726 = 0.29274M

[H3O^+] = x = 0.00726M

[HCOO^-] = x = 0.00726M

[OH-] = Kw/[H3O^+]

= 1*10^-14/0.00726 = 1.37*10^-12M

PH = -log[H3O+]

= -log1.37*10^-12 = 11.86 >>>>answer

b.

HCOOH(aq) + H2O(l)--------------> H3O+(aq) + HCOO–(aq)

I 0.005 0 0

C -x +x +x

E 0.005-x +x +x

Ka = [H3O^+][HCOO^-]/[HCOOH]

1.8*10^-4 = x*x/0.005-x

1.8*10^-4 *(0.005-x) = x^2

x= 0.000863

[HCOOH] = 0.005-x = 0.005-0.000863 = 0.004137M

[H3O^+] = x = 0.000863M

[HCOO^-] = x = 0.000863M

[OH-] = Kw/[H3O^+]

= 1*10^-14/0.000863 = 1.158*10^-11M

PH = -log[H3O+]

= -log0.000863 = 3.0639 >>>>answer

queen_honey_blossom answered 1 year ago

What is the pH of 0.005 M Ba(OH)2 solution? a) 12 b) 2 c) 0.005 d)...

What is the pH of 0.005 M Ba(OH)2 solution? a) 12 b) 2 c) 0.005 d) -2

Calculate the pH, pOH, [H3O+], and [OH-] of the following solutions: (a) 0.001 M HNO3, (b)...

Calculate the pH, pOH, [H3O+], and [OH-] of the following solutions: (a) 0.001 M HNO3, (b) 0.3 M Ca(OH)2; (c) 3.0 M HNO3, (d) 6.0 M NaOH, (e) 0.05 M HBr

For each strong acid solutions, determine [H3O+],[OH−], and pH. a) 0.20 M HCl b) pH c)...

For each strong acid solutions, determine [H3O+],[OH−], and pH. a) 0.20 M HCl b) pH c) 2.5×10−2 M HNO3 d) pH

(a) What are [H3O+], [OH -], and pOH in a solution with a pH of 2.49?...

(a) What are [H3O+], [OH -], and pOH in a solution with a pH of 2.49? [H3O]....................... POH......................... PH............................. (b) What are [H3O+], [OH -], and pH in a solution with a pOH of 5.99? [H3O].................... POH...................... PH.........................

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. A)8.89×10−3 M LiOH [OH−],[H3O+] =...

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. A)8.89×10−3 M LiOH [OH−],[H3O+] = b)8.89×10−3 M LiOH pH,pOH= C)1.15×10−2 M Ba(OH)2 [OH−],[H3O+]= D)1.15×10−2 M Ba(OH)2 pH,pOH = E)1.8×10−4 M KOH [OH−],[H3O+]= F)1.8×10−4 M KOH pH,pOH = G)4.9×10−4 M Ca(OH)2 [OH−],[H3O+] = H)4.9×10−4 M Ca(OH)2 pH,pOH =

Construct a spreadsheet that has the following column headings: pH [H3O+] [OH-] log [H3O+] log [OH-]...

Construct a spreadsheet that has the following column headings: pH [H3O+] [OH-] log [H3O+] log [OH-] Under “pH” enter the range for 0-14 in 0.1 increments. (Use the “FILL” com- mand to make it easier.) Under “[H3O+]” enter =10^-pH where you will provide the cell address for “pH” (cell addresses that you must enter are shown in italics). Recall that the “=“ symbol indicates that a formula follows, while the “^” symbol signifies an exponent. Under “[OH-]”, enter =10^-14 /...

What are the concentrations of H3O+ and OH- in each of the following? a. 1.55 M...

What are the concentrations of H3O+ and OH- in each of the following? a. 1.55 M NaOH b. 0.15 M Sr(OH)2 c. 0.056 M HClO4 d. 0.47 M HCl

Calculate [H3O+] and [OH−] for each of the follo... pH= 8.56 pH= 11.20 pH= 2.84

Calculate the pH of each solution. A. [H3O+] = 7.7×10−8 M B. [H3O+] = 4.0×10−7 M...

Calculate the pH of each solution. A. [H3O+] = 7.7×10−8 M B. [H3O+] = 4.0×10−7 M C. [H3O+] = 3.2×10−6 M D. [H3O+] = 4.4×10−4 M

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. in part A,B,and C A.)...

For each strong base solution, determine [H3O+], [OH−], pH, and pOH. in part A,B,and C A.) 8.78×10−3 M LiOH Express your answer using three significant figures. Enter your answers numerically separated by a comma. [OH−],[H3O+] = M B.)5.3×10−4 M Ca(OH)2 Express your answer using two significant figures. Enter your answers numerically separated by a comma. [OH−],[H3O+] = M C.) 5.3×10−4 M Ca(OH)2 Express your answer to two decimal places. Enter your answers numerically separated by a comma. pH,pOH = D.)...