MCQ
At ${25\,^o}C$ Ethylene glycol is a
- ASolid compound
- ✓Liquid
- CGas
- DBrown solid
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$C{{H}_{3}}-C\equiv CH\xrightarrow[{{H}_{2}}S{{O}_{4}}]{HgS{{O}_{4}}}A\xrightarrow{NaB{{H}_{4}}}B$
| Column $-I$ (various solutions) | Column $-II$ (Their freezing point ) | ||
| $a$ | $0.1\,M\, BaCl_2$ solution | $p$ | $271\,K$ |
| $b$ | $0.1\,M\, NaCl$ solution | $q$ | $270\, K$ |
| $c$ | $0.1\,M\, K_3 [Fe(CN)_6]$ solution | $r$ | $268\, K$ |
| $d$ | $0.1\,M\, Al_2 (SO_4)_3$ solution | $s$ | $269\, K$ |
Given : Freezing point of $0.1\,M$ sucrose solution $= 272\,K$ and $F.pt.$ of water $= 273\,K$
Which of the following option show correct matches ? (assume, molarity=molality)
Reason : Oxidation state of $Cl$ in $HClO_4$ is $+VII$ and in $HClO_3$ $+V$.
The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$, the rate becomes $100$ times when $pH$ is decreased from $3\, to\, 2$. Identify the correct statements $(pH = -\log [H^{+}])$
$(A)$ $\frac{{dx}}{{dt}}\, = k{[Zn]^0}{[{H^ + }]^2}$
$(B)$ $\frac{{dx}}{{dt}}\, = k{[Zn]}{[{H^ + }]^2}$
$(C)$ Rate is not affected if the concentraton of zinc is made four times and that of $H^+$ ion is halved.
$(D)$ Rate becomes four times if the concentration of $H^+$ ion is doubled at constant $Zn$ concentration