Advertisements
Advertisements
प्रश्न
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Advertisements
उत्तर
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
संबंधित प्रश्न
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
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.
The pH of 10−8 M of HCl is ______.
In NaOH solution [OH–] is 2.87 × 10–4. Calculate the pH of the solution.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
The least basic hydroxide from the following is:
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
In which of the following solvents is silver chloride most soluble?
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
Assertion (A): Increasing order of acidity of hydrogen halides is \[\ce{HF < HCl < HBr < HI}\]
Reason (R): While comparing acids formed by the elements belonging to the same group of periodic table, \[\ce{H - A}\] bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
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 pH.
Define pOH.
Derive the relation pH + pOH = 14.
Derive the relation pH + pOH = 14.
Define pH.
Define the following term:
pOH
