Home
Class 12
CHEMISTRY
In the titration of NH(4)OH versus HCl, ...

In the titration of `NH_(4)OH` versus `HCl`, the `pH` of the solution at equivalence point is about:

A

about `5.5`

B

about 7

C

about `8.5`

D

about `9.5`

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise IN - CHAPTER EXERCISE - A|10 Videos
  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise IN - CHAPTER EXERCISE - B|10 Videos
  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise PRACTICE EXERCISE - 5|5 Videos
  • INTRODUCTION TO ORGANIC CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE ADVANCED ARCHIVE|81 Videos
  • JEE MAIN - 5

    VMC MODULES ENGLISH|Exercise PART II : CHEMISTRY (SECTION - 2)|5 Videos

Similar Questions

Explore conceptually related problems

In the titration of NH_(4)OH) with HCl, the indicator which cannot be used is :

100 ml of 0.2 M CH3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be (pKa of CH3COOH=4.76)

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

10 mL of H_(2)A (weak diprotic acid) solution is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at first equivalence point is pH_(1) and at second equivalence point is pH_(2^.) Calculate the value of (pH_(2)-pH_(1)) at 25^(@)C Given for H_(2)A,pK_(a_1) =4.6 and pK_(a_2) =8, log 25=1.4

10 mLof H2A (weak diprotic acid) solutions is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at 1^(st) equivalence point is pH_(1) and at 2^(nd) equivalence point is pH_(2) , Cal the value (pH_(2),-pH_(1)) at 25^(@) C. Given for H_(2),A, p^(Kal) =4.6 &p^(Ka2) =8

20 ml of 0.1 M ' NH_3', solution is titrated with 0.025M HCI solution. What is the pH of the reaction mixture at equivalence point at 25^(@) C ? (K_(b) "of " NH_(3) "is " 2 xx 10^(-6)) .

An aqueous solution of HCl is 10^(-9) M HCl . The pH of the solution should be

The equivalent conductances of an infinitely dilute solution NH_(4)CI is 150 and the ionic conductances of OH^(-) and CI^(-) ions are 198 and 76 respectively. What will be the equivalent conductance of the solution of NH_(4)OH at infinite dilution. if the equivalent conductance of a 0.01N solution NH_(4)OH is 9.6, what will be its degree of dissociation.

When weak base solution (50mL of 0.1 N NH_(4)OH) is titrated with strong acid (0.1N HCI) , the pH of the solution initially decrease fast and then decreases slowely till near the equivalence point (as shown in figure). Which of the following is//are correct.

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid and base react rapidly to neutralize each other. At the equivalence point, equivalents of reacting substances are equal. The pH during a titration changes every time with a drop of titrant added, but the rate of this change varies enormously. A titration curve, graph of pH as a function of the volume of titrant, displays in detail how the pH changes over the course of an acid base titration. Significantly. the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K_(a) and K_(b) of acid and base The pH at equivalence point is: