What is the pH of a solution of 1.00L of water with 0.00527 moles of HCl in it ?
ID: 974504 • Letter: W
Question
What is the pH of a solution of 1.00L of water with 0.00527 moles of HCl in it ?
What is the pH of a solution of 1.00L of water with 0.0165 moles of HNO3 in it ?
What is the pH of a solution of 1.00L of water with 0.0823 moles of NaOH in it ?
What is the pH of a solution of 1.00L of water with 0.0815 moles of KOH in it ?
Based on the definitions for strong acid and weak acid, would you expect the concentration of an acid to play a role in determining if it's strong or weak? Explain your answer. Be specific.
In the neutralization reaction
H2SO4 + 2 KOH à 2 H2O + K2SO4
If there is 850 mL of 0.128 M H2SO4 reacting with 470 mL of a KOH solution with unknown concentration, what is the concentration of KOH?
Explanation / Answer
pH of HCl = 2.28
pH of HNO3 = 1.78
pH of NaOH = 12.92
pH of KOH = 12.91
Concentration will not play on strength of acids. it depend how easily ( or what extend) dissociates in solvent or solution. If it completely dissociate , that will be strong acid, if partially dissociate then that will be weak acid.
H2SO4 + 2 KOH à 2 H2O + K2SO4 in this reaction H2SO4 and KOH both are completely dissociates and forms K2SO4 salt so both are termed as strong
850 mL of 0.128 M H2SO4 = 108.8 mmol of H2SO4
1 eq of acid will react with 2 eq of KOH so we need 217.6 mmol of KOH in 470 mL
0.2176 mole / 0.470 L = 0.463 M concentration of KOH 470 mL needed.
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