ANSWERS-
9 gm of NaOH is added to 3L water,
Molarity = moles/volume
Moles of NaOH= mass / molar mass = 9/40 = 0.225 moles
NaOH = Na+ + OH-
As 1 mole NaOH gives 1 mole OH- thus 0.225 moles NaOH gives 0.225 moles of OH-
Molarity of OH- = 0.225/3 = 0.075 M
p[OH] = -log(OH-) = -log(0.075) = 1.125
pH = 14-pOH = 14-1.125 = 12.875
and as [OH-] × [H+] = 10^-14,
thus, [H+] = 1.333 × 10^-13
Review Problem 16.065 A sodium hydroxide solution is prepared by dissolving 9.0 g NaOH in 3.00...
Review Problem 16.066 A solution was made by dissolving 0.818 g Ca(OH)2 in 100 ml final volume. (Note: For the purpose of significant figures, assume Kw - 1.00 x 10" (a) What is the molar concentration of OH" in the solution? (OH) - (b) What is the pH? pH- (c) What is the pOH? рон (d) What is the hydrogen ion concentration in the solution? (H) - Click if you would like to Show Work for this question: Open Show...
Review Problem 16.066 Your answer is partially correct. Try again. A solution was made by dissolving 0.897 g Ca(OH)2 in 100. mL final volume. (Note: For the purpose of significant figures, assume Kw = 1.00 x 10" 14) (a) What is the molar concentration of OH in the solution? [OH-] = 1.159 (b) What is the pH? pH 713.204 (c) What is the pOH? pOH = .795 (d) What is the hydrogen ion concentration in the solution? [H+] = 46.25e-14
A sodium hydroxide solution is prepared by 8.56 g in 2.25 L of solution. What is the molarity of the OH- in the solution? What is the pOH, pH, and [H+] of the solution?
What is the molarity of sodium hydroxide (NaOH) in a solution prepared by dissolving 100 g of the solute into 1000 mL of solution?
pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH = -log[H+]Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the Kw of water: Kw = [H+][OH-] = 1.00 x 10-14where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 = pH...
NA Review | Constants 1 Periodic Table pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: The temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10-14. pH = -log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the Kw of water: Part A Kw = [H+][OH-] =...
A solution was made by dissolving 1.77 g Ba(OH)2 in 100. mL final volume. (Note: Kw = 1.00 x 10-14) (a) What is the molar concentration of OH- in the solution? (b) What is the pH? (c) What is the pOH? (d) What is the hydrogen ion concentration in the solution?
pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10−14 where 1.00×10−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH Part B Part complete 0.25 g of...
pH of a Strong Acid and a Strong Base 11 of 16 > II Review Constants Periodic Table pH is a logarithmic scale used to indicate the hydrogen ion concentration, H'], of a solution: pH = -log[H] The temperature for each solution is carried out at approximately 297 K where Ky = 1.00 x 10-14 Part A Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, OH-], are related to...
5. (10 pts) Find pH of solution prepared by dissolving 1.0 g of sodium carbonate and 1.0 g of sodium hydrogen carbonate in enough water to make 100.0 mL solution. The base dissociation constant of carbonate ion is 1.8x10-4. Assume that hydrogen carbonate ion does not react with water.