Advertisements
Advertisements
Question
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Advertisements
Solution
Moles of `"H"_3"O"^+ = (2xx 10 xx 0.01)/1000` = .0002 mol
Moles of `"OH"^- = (2xx10xx 0.01)/1000 = .0002 "mol"`
Since there is neither an excess of `"H"_3"O"^ or "OH"^-`, the solution is neutral. Hence, pH = 7.
APPEARS IN
RELATED QUESTIONS
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Answer the following in one sentence :
Calculate the pH of 0.01 M sulphuric acid.
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
Calculate the pH of 0.04 M HNO3 solution.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Neutral solutions have the pH of ______.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Derive the relationship between pH and pOH.
Derive relationship between pH and pOH.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Define pH.
Define the following term:
pOH
