MCQ
The $pH$ of a solution is $5.0$. To this solution sufficient acid is added to decrease the $pH$ to $2.0$. The increase in hydrogen ion concentration is.....$times$
- A$100$
- B$10$
- ✓$1000$
- D$2.5$
When $pH =5$,
$\left[ H ^{+}\right]=10^{- pH }=10^{-5}\, M$
The $pH$ of solution is decreased to $2 .$
When $pH =2$,
$\left[ H ^{+}\right]=10^{- pH }=10^{-2} \,M$
The change in concentration of $\left[ H ^{+}\right]$is $10^{-2} / 10^{-5}=10^3=1000.$
It is increased by $1000$ times.
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$(I)\,[Kr]\,5s^1$ $(II)\, [Rn]\,5f^{14}\,6d^1\,7s^2$
$(III)\,[Ar]\,3d^{10}\,4s^2\,4p^5$ $(IV)\,[Ar]\,3d^6\,4s^2$
Consider the following Statements
$(i)\, I$ shows variable oxidation State
$(ii)\, II$ is a $d-block$ element
$(iii)$ The compound formed between $I$ and $III$ is covalent
$(iv)\,IV$ shows single oxidation state
Which Statement is True $(T)$ or False $(F)$?