Calculate the [H3O+] and pH of each polyprotic acid solution. (See the appendix.)
(a) 0.272 M H2CO3
[H3O+] | M |
pH |
(b) 0.133 M
H3C6H5O7
[H3O+] | M |
pH |
Ans a) H2CO3 is a weak acid
H2CO3 +H2O
H3O+ +HCO3-
H2CO3 | H3O+ | HCO3- | |
initial | 0.272 | 0 | 0 |
change | - x | x | x |
equilibrium | 0.272-x | x | x |
Here Ka = 4.3 x 10-7
4.3 x 10-7 = x2 / 0.272-x
x=0.645
[H3O+] = 0.645
pH= - log[H3O+]
= 3.89
Ans;- b) H3C6H5O7 +
H2O
H3O+ +
C6H5O7-
Here Ka = 6.46 x 10-5
H3C6H5O7 | H3O+ | C6H5O7- | |
initial | 0.133 | 0 | 0 |
change | - x | +x | +x |
equilibrium | 0.133-x | x | x |
6.46 x 10-5 = x2 / 0.133- x
x = 0.00110
[H3O+] = 0.00110
pH= - log[H3O+]
= 2.95
Calculate the [H3O+] and pH of each polyprotic acid solution. (See the appendix.) (a) 0.272 M...
Part A Calculate the [H3O+] of the following polyprotic acid solution: 0.115M H2CO3. Part B Calculate the pH of this solution. Part C Calculate the [H3O+]] of the following polyprotic acid solution: 0.145M H3C6H5O7. Part D Calculate the pH of this solution.
Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.145 M H3C6H5O7
1. Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.400 M H3PO4. Calculate the pH of this solution. 2. Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.400 M H2C2O4.
Part A= Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.300 M H2C2O4. Part B= Calculate the pH of this solution.
Calculate the [H3O+]and pH of the following polyprotic acid solution: 0.300 M H2C2O4. Part D Calculate the pH of this solution.
Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.350 M H2C2O4.
Part A= Calculate the [H3O+] of the following polyprotic acid solution: 0.350 M H3PO4. Part B= Calculate the pH of this solution. Part C= Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.300 M H2C2O4. Part D= Calculate the pH of this solution.
Calculate the pH and concentration of species present in a polyprotic acid solution.For a 3.44×10-3 M solution ofH2CO3, calculate both the pH and the CO32- ion concentration.H2CO3 + H2O → H3O+ +HCO3-Ka1 = 4.2×10-7HCO3- + H2O → H3O+ +CO32-Ka2 = 4.8×10-11pH =[CO32-] =
Calculate the [H3O+] of the following polyprotic acid solution: 0.310 MH3PO4 .Express your answer using two significant figures. Part B Calculate the pH of this solution. Express your answer using one decimal place.
What is a polyprotic acid? 2. How many moles of H3O + are present in 50 mL of 0.3 M H2SO4? 4. If 20.20 mL of 0.122 M NaOH are required to reach the first equivalence point of a solution of citric acid (H3C6H5O7), how many mL of NaOH are required to completely neutralize this solution? 5. If the pH at one-half of the neutralization points of a dibasic acid is 3.52 and 6.31 respectively, what are the values for...