Home
Class 12
CHEMISTRY
Buffer solution have constant acidity an...

Buffer solution have constant acidity and alkalinity because :
1. these give unionised acid or base on reaction with added acid and bases
2. acids and alkalies in these solution are shielded from attack by other ions
3. they have large excess of `H^(+) or OH^(-) ` ions
4. they have fixed value of pH

A

They have large excess of `H^(+) or OH^(-)` ions

B

They have fixed value of pH

C

These give unionised acid or base on reaction with added acid or alkali

D

Acids and alkalies in these solutions are shielded from attack by other ions

Text Solution

Verified by Experts

The correct Answer is:
C

These give unionised acid or base on reaction with added acid or alkali
Promotional Banner

Similar Questions

Explore conceptually related problems

How is that in alkaline solution we have chromate and in acidic solution dichromates ? Give their structures.

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid /base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) What is DeltaH^(@) for complate neutralization of strong diacidic base A(OH)_(2)by HNO_(3) ?

A buffer solution contains a weak acid HA and A . When small quantity of NaOH is added, to keep p^(H) as constant. which of the following reaction takes place?

Enthalpy of neutralzation is defined as the enthalpy change when 1 mole of acid // base is completely neutralized by base // acid in dilute solution . For Strong acid and strong base neutralization net chemical change is H^(+) (aq)+OH^(-)(aq)to H_(2)O(l) Delta_(r)H^(@)=-55.84KJ//mol DeltaH_("ionization")^(@) of aqueous solution of strong acid and strong base is zero . when a dilute solution of weak acid or base is neutralized, the enthalpy of neutralization is somewhat less because of the absorption of heat in the ionzation of the because of the absorotion of heat in the ionization of the weak acid or base ,for weak acid /base DeltaH_("neutrlzation")^(@)=DeltaH_("ionization")^(@)+ Delta _(r)H^(@)(H^(+)+OH^(-)to H_(2)O) under same conditions ,how many mL of 0.1 m NaOH and 0.05 M H_(2)A (strong diprotic acid ) solution should be mixed for a total volume of 100mL to producce the hight rise in temperature ?

The pH of a 0.1 molar solution of the acid HQ is 3 . The value of the ionisation constant, K_(a) of the acid is

The pH of a 0.1 molar solution of the acid HQ is 3 . The value of the ionisation constant, K_(a) of the acid is

The ionization constant of a certain weak acid is 10^(-4) . What should be the [salt] to [acid] ratio if we have to prepare a buffer with pH = 5 using this acid and one of the salts

Calculate the concentration of hydrogen ion in the acidic solution with pH a. 4.3

The pH of a solution is 5. to this solution acid was added so that its pH value bcomes 2.0. The increase in H^(+) concentration is :

The dissociation constant of a weak acid is 1 xx 10^(-4) . In order of prepare a buffer solution with a pH =5 the [Salt]/[Acid] ratio should be