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Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :
a. $60 mL\dfrac{M}{10}HCL+40 mL\dfrac{M}{10} NaOH$
b. $55 mL\dfrac{M}{10}HCL+45 mL\dfrac{M}{10} NaOH$
c. $75 mL\dfrac{M}{5}HCL+25 mL\dfrac{M}{5} NaOH$
d. $100 mL\dfrac{M}{10}HCL+100 mL\dfrac{M}{10} NaOH$
pH of which one of them will be equal to 1?
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On which of the following properties does the coagulating power of an ion depend?
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Given van der Waals constant for $NH_3, H_2, O_2$ and $CO_2$ are respectively 4.17, 0.244, 1.36 and 3.59, which one of the following gases is most easily liquefied?
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The solubility of $BaSO_4$ in water is 2.42 × $10^{–3} gL^{–1}$ at 298 K. The value of its solubility product $(K_{sp})$ will be
(Given molar mass of
$BaSO_4 = 233 g mol–1)$
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In which case is number of molecules of water maximum?
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The correct difference between first and second order reactions is that
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Among $CaH_2, BeH_2 , BaH_2,$ the order of ionic character is
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Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below :
Then the species undergoing disproportionation is
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For the redox reaction
$MnO_4^-+C_2O_4^{2-}+H^+\rightarrow Mn^{2+} +CO_2 + H_2O$
The correct coefficients of the reactants for the balanced equation are
$MnO_4^-$ $C_2O_4^{2-}$ $H^+$
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Which one of the following conditions will favour maximum formation of the product in the reaction,
$A_2(g)+B_2(g)\rightleftharpoons X_2(g)\triangle_r H=-XKJ?$
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