find pH 2. [OH-] = 7.42 x 10-5 M odlo a TO

Question

Question

find pH

science chemistry

Answer 1

Answer #1

& ot given, firstly the From the concentration of pot is calculated, POH - - log [54] - log (7.928105) - 4.129 PH related as

Answer 2

Similar Homework Help Questions

5. What is the pH of a solution with a OH concentration of 2.52 x 10'M?...

5. What is the pH of a solution with a OH concentration of 2.52 x 10'M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 6. What is the pH of a solution with a H2O* concentration of 2.7 x 10 M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 7. What is the pH of a solution with a OH concentration of 5.53 x 10-M? Is this solution...
Calculate pH part a) [OH-] = 8.9 x 10^-7 M part b) [OH-] = 7.6 x...

Calculate pH part a) [OH-] = 8.9 x 10^-7 M part b) [OH-] = 7.6 x 10^-8 M part c) [OH-] = 6.2 x 10^-11 M part d) [OH-] = 1.5 x 10^-2 M
Calculate the pH of each of the following solutions. (a) 1.3 x 10-4 M Ba(OH)2: x...

Calculate the pH of each of the following solutions. (a) 1.3 x 10-4 M Ba(OH)2: x 10 (Enter your answer in scientific notation.) (b) 1.7 x 10-4 M HNO3: Calculate the pH of a 0.025 M CHEN (pyridine) solution. The K, for pyridine is 1.7 x 10 9. pH =

A. Find "[OH-]= ____ M" for 5.0x10-2 M NaBrO. B. Find the pH for part A....

A. Find "[OH-]= ____ M" for 5.0x10-2 M NaBrO. B. Find the pH for part A. C. Find [OH-] = ___ M" for a mixture that is 0.12 M in NaNO2 and 0.15 M in Ca(NO2)2. D. Find the pH for part C.
A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution....

A solution has [OH-] = 4.33 x 10-5 M. Calculate [H3O+] and pH of the solution. Then, tell whether the solution is acidic, basic, or neutral. Also, calculate pOH.
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-] =...

2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-]...

2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
Calculate Ka for 1 M NaCH3COO pH = 9.37 H+ = 4.203 X 10^-10 OH- =...

Calculate Ka for 1 M NaCH3COO pH = 9.37 H+ = 4.203 X 10^-10 OH- = 2.402 X 10^-5 CH3COO- = 1.00 X 10^0 CH3COOH = 2.402 X 10^-5 ________________ Calculate Ka using the formula Kw = Ka X Kb and the appropriate equilibrium constant for 1 M NaCH3COO. NaCH3COO ---> Na+ (neutral) + CH3COO-. Is the conjugate base for CH3COOH. CH3COOH Ka1 = 1.8 X 10^-5 ______________________ Calculate Ka for 1 M NH4Cl pH = 4.26 H+ = 2.336...
Calculate the [OH-] and the pH of a solution with an [H+] = 4.8 x 10-6 M at 25 °C.

Calculate the [OH-] and the pH of a solution with an [H+] = 4.8 x 10-6 M at 25 °C.Calculate the [H+] and the pH of a solution with an [OH-] = 8.8 x 10-13 M at 25°C. Calculate the [H+] and the [OH-] of a solution with a pH = 11.04 at 25°C.

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...