Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 11.11. Express...

Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 11.11.

Express your answer using two significant figures.

[Ca(OH)2] =

M

SubmitMy AnswersGive Up

Expert Solution

queen_honey_blossom answered 2 years ago

Using the aqueous equilibrium constants, calculate the concentration of OH- in M and pH for the...

Using the aqueous equilibrium constants, calculate the concentration of OH- in M and pH for the following solutions (given that all are at 25 degrees celsius): 0.15 M NaBrO 8.2×10−2 M NaHS. A mixture that is 0.13 M in NaNO2 and 0.25 M in Ca(NO2)2. Thank you! :)

Calculate the OH- concentration and pH of a 3.7×10-3M aqueous solution of sodium cyanide, NaCN. Finally,...

Calculate the OH- concentration and pH of a 3.7×10-3M aqueous solution of sodium cyanide, NaCN. Finally, calculate the CN- concentration. Ka (HCN) = 4.9×10-10.

Calculate the [H3O+] of each aqueous solution with the following [OH−] . Express your answer using...

Calculate the [H3O+] of each aqueous solution with the following [OH−] . Express your answer using two significant figures. 1.Vinegar, 1.2 x 10-11M, Express your answer using two significant figures. 2. Urine, 2.3x10-9 M, Express your answer using two significant figures. 3. Ammonia, 5.8×10−3 M, Express your answer using two significant figures. 4. NaOH, 4.0×10−2 M, Express your answer using two significant figures.

Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically...

Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of NaOHNaOH. Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of hydrazine, N2H4. Kb for hydrazine is 1.3×10−61.3×10−6. Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of hypochlorous acid, HOCl. Ka of HOCl is 3.5×10−8. Express...

What is the solubility of Mg(OH)2 in an aqueous solution buffered to a pH of 13.13?...

What is the solubility of Mg(OH)2 in an aqueous solution buffered to a pH of 13.13? The Ksp of Mg(OH)2 is 1.8 x 10-11. Hint: Determine the [OH-] from the pH then deal with solubility with common ion. Determine if adding each of the following to a saturated Ca3(PO4)2 solution will increase, decrease, or have little to no effect on it ssolubility. - A. B. C. HCl - ...

A. Calculate [H3O+] in the following aqueous solution at 25 ?C: [OH?]= 1.6×10?9 M . Express...

A. Calculate [H3O+] in the following aqueous solution at 25 ?C: [OH?]= 1.6×10?9 M . Express your answer using two significant figures. B. Calculate [H3O+] in the following aqueous solution at 25 ?C: [OH?]= 3.0×10?2 M . Express your answer using two significant figures. C. Calculate [H3O+] in the following aqueous solution at 25 ?C: [OH?]= 7.0×10?12 M . Express your answer using two significant figures.

What is the solubility of Mg(OH)2(s) in an aqueous solution of pH 13.00 at 25oC? The...

What is the solubility of Mg(OH)2(s) in an aqueous solution of pH 13.00 at 25oC? The solubility product of Mg(OH)2(s) at this temperature is 1.2 x 10-11. (Answer: 8.7 x 10-8 g/L)

Calculate the [OH−] of each aqueous solution with the following [H3O+]: stomach acid, 2.0×10−2M Express your...

Calculate the [OH−] of each aqueous solution with the following [H3O+]: stomach acid, 2.0×10−2M Express your answer using two significant figures. urine, 7.0×10−6M Express your answer using two significant figures. orange juice, 2.2×10−4M Express your answer using two significant figures. bile, 6.0×10−9M Express your answer using two significant figures.

A) A solution of Ba(OH)2 has a molarity of 0.00617 mol/L. Calculate the final pH of...

A) A solution of Ba(OH)2 has a molarity of 0.00617 mol/L. Calculate the final pH of the solution. B) Consider the reaction: CaBr2(s) → Ca(s) + Br2(l) Which of the following statements is correct? Select all that apply. Bromide Ion is reducing agent NOT a spontaneous reaction Ca is oxidized Br is Oxidized Br is Reduced Ca is Reduced Calcium Ion is the Reducing Agent IS a spontaneous reaction Br ion is the oxidizing agent. Ca ion is the oxidizing...

Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.99? The Ksp of Fe(OH)2 is 4.87

Question