(A) When $KBr$ is dissolved in water,it dissociates into $K^{+}$ and $Br^{-}$ ions. These ions interact with water molecules through ion-dipole intera

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(A) When $KBr$ is dissolved in water,it dissociates into $K^{+}$ and $Br^{-}$ ions. These ions interact with water molecules through ion-dipole interactions,a process known as hydration.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Water hydrolysis and pH scale

Easy

When $KBr$ is dissolved in water,$K^{+}$ ions are

KCET 2007 All KCET

A
hydrated
B
hydrolysed
C
reduced
D
oxidised

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

6-2.Equilibrium-II (Ionic Equilibrium)

Subtopic

Water hydrolysis and pH scale

Previous Year

KCET 2007 Paper All KCET years →

$100 \ mL$ of $NaOH$ solution has a $pH = 10$. Calculate the concentration of hydroxide ions,$[OH^{-}]$.

Easy

View Solution

Hydrogen ion concentration in $mol/L$ in a solution of $pH = 5.4$ will be

MediumAIEEE 2005

View Solution

$A$ $pH$ of $7$ signifies

Easy

View Solution

At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

Medium

View Solution

At $100\, ^oC$,the $K_w$ of water is $55$ times its value at $25\, ^oC$. What will be the $pH$ of a neutral solution at this temperature? $(\log 55 = 1.74)$

DifficultNEET 2013

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

When $KBr$ is dissolved in water,$K^{+}$ ions are

Similar Questions

$100 \ mL$ of $NaOH$ solution has a $pH = 10$. Calculate the concentration of hydroxide ions,$[OH^{-}]$.

Hydrogen ion concentration in $mol/L$ in a solution of $pH = 5.4$ will be

$A$ $pH$ of $7$ signifies

At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

At $100\, ^oC$,the $K_w$ of water is $55$ times its value at $25\, ^oC$. What will be the $pH$ of a neutral solution at this temperature? $(\log 55 = 1.74)$

Vedclass Test Series

Exam Paper Generator

Online Exam Module