Equal volumes of $10 %$ (v/v) of $H C l$ is mixed with $10 %$ (v/v) $N a O H$ solution. If density of pure $N a O H$ is $1.5$ times that of pure $H C l$ , then the resultant solution will be :

basic

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neutral

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acidic

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can't be predicted

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Solution

The correct option is A basic
Since the density of pure $N a O H$ is $1.5$ times that of pure $H C l$ and the volumes (and volume percent) are equal, the mass (and moles) of $N a O H$ will be $1.5$ times that of $H C l$ .
$N a O H$ is in excess.
Therefore, the resultant solution will be basic.

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Equal volumes of 10% (v/v) of HCl is mixed with 10% (v/v) NaOH solution. If density of pure NaOH is 1.5 times that of pure HCl, then the resultant solution will be :

The correct option is A basicSince the density of pure NaOH is 1.5 times that of pure HCl and the volumes (and volume percent) are equal, the mass (and moles) of NaOH will be 1.5 times that of HCl.NaOH is in excess. Therefore, the resultant solution will be basic.

Equal volumes of $10 %$ (v/v) of $H C l$ is mixed with $10 %$ (v/v) $N a O H$ solution. If density of pure $N a O H$ is $1.5$ times that of pure $H C l$ , then the resultant solution will be :

The correct option is A basic
Since the density of pure $N a O H$ is $1.5$ times that of pure $H C l$ and the volumes (and volume percent) are equal, the mass (and moles) of $N a O H$ will be $1.5$ times that of $H C l$ .
$N a O H$ is in excess.
Therefore, the resultant solution will be basic.