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:
0.002 M KOH
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Define pH.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Calculate the pH and pOH of 0.0001 M HCl solution.
Which of the following is INCORRECT statement?
The pH of a monoacidic weak base is 11.5. The concentration of OH− ions in this solution is ____________ M.
Aqueous solution of ____________ will turn red litmus blue.
The least basic hydroxide from the following is:
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Neutral solutions have the pH of ______.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Define pOH.
Define pOH.
Define pOH.
Define pH.
Define pOH.
Define the following term:
pH
Which from the following compound in aqueous medium having minimum pH?
