Home
Class 12
CHEMISTRY
The active ingredients in aspirin is ac...

The active ingredients in aspirin is acetly salicylic acid

with `K_(a) = 2.75 xx10^(-9)` , The pH of the solution obtained by dissolving twoe aspirin tablets (containing 0.32 g of acetyl salicylic acid in eac tablet ) in 250 ml of water is (given log `6.25 = 0.80` )

A

`5.20`

B

`4.20`

C

`3.20`

D

`7.20`

Text Solution

Verified by Experts

Promotional Banner

Similar Questions

Explore conceptually related problems

Accetyl salicylic acid (aspirin) ionises in water as: (K_(a) = 2.75 xx 10^(-9)) If two tablets of aspirin each of 0.32g is dissolved in water to produce 250mL solution, calculate

The acid dissociation constant of uric acid is K_(a)=4.0xx10^(-6) M. The pH of a sample of urine is 6.0. What is the ratio of concentration of urate ion to uric acid in the urine? (a) 2.0 (b) 4.0 (c) 6.0 (d) 0.25

Calculate degree of hydrolysis(h) and pH of solution obtained by dissolving 0.1 moles of CH_(3)COOHNa in water to get 100L of solution .Take K_(a) of acetic acid =2xx10^(-5) at 25^(@)C .

Calculate the pH of buffer solution prepared by dissolving 0.20 mol of sodium cyanate (NaCNO) and 1.0 mol of cynic acid (HCNO)in enough water to make 1.0 litre of solution . K_a(HCNO)=2.0 xx10^(-4)

10 ml of 0.2 M acid is added to 250 ml of a buffer solution with pH = 6.34 and the pH of the solution becomes 6.32 . The buffer capacity of the solution is :

What will be the hydrogen ion concentration of a solution obtained by mixing 500 ml of 0.20 M acetic acid 500 ml of 0.30 M sodium acetate (K_(a) = 1.75 xx 10^(-5))

When NaOH solution is gradually added to the solution of weak acid (HA), the pH of the solution is found to be 5.0 at the addition of 10 and 6.0 at further addition of 10 ml of same NaOH. (Total volume of NaOH =20ml). Calculate pK_(a) for HA. [log2 = 0.3]

What is the pH of a solution obtained by dissolving 0.0005 mole of the strong electrolyte, calcium hydroxide, Ca(OH)_(2) , to form 100 ml of a saturated solution (aqueous)? (K_(w)=1.0 xx 10^(-14) "mole"^(2) "litre"^(-2))

100mL of a buffer solution contains 0.1M each of weak acid HA and salt NaA . How many gram of NaOH should be added to the buffer so that it pH will be 6 ? (K_(a) of HA = 10^(-5)) .

The concentration of hydrogen ions in a 0.2M solution of formic acid is 6.4 xx 10^(-3) mol L^(-1) . To this solution, sodium formate is added so as to adjust the concentration of sodium formate to 1 mol L^(-1) . What will be the pH of this solution? The dissociation constant of formic acid is 2.4 xx 10^(-4) and the degree of dissociation fo sodium formate is 0.75 .