Advertisements
Advertisements
Question
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Advertisements
Solution
For 0.3 g of NaOH dissolved in water to give 200 mL of solution:
\[\ce{NaOH -> Na^+_{(aq)} + OH^-_{(aq)}}\]
`["NaOH"] = 0.3 xx 1000/200 = 1.5 "M"`
`["OH"_("aq")^-] = 1.5 "M"`
Then `["H"^+] = 10^(-14)/1.5`
`= 6.66 xx 10^(-13)`
`"pH" = - log(6.66 xx 10^(-13))`
= 12.18
APPEARS IN
RELATED QUESTIONS
The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Calculate the pH and pOH of 0.0001 M HCl solution.
The CORRECT match between transition metal ion and its colour in aqueous solution.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
Which of the following is CORRECT for an aqueous solution of NH4CN?
[Ka of HCN = 4.0 × 10−10, Kb for NH4OH = 1.8 × 10−5]
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
The pH of an aqueous solution is Zero. The solution is ____________.
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?
A sample of air turns lime water milky and also turns acidified potassium dichromate green in aqueous solution has low pH. This is due to the presence of pollutants.
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
Define pOH.
Define pH.
Define pH.
Derive the relation pH + pOH = 14.
Define pOH.
Which from the following compound in aqueous medium having minimum pH?
