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Question #e0bf1

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Apr 28, 2017

We have $15 \times 0.2 = 3.0 m m o l$ $15xx0.2=3.0mmol$ reacting with $10 \times 0.15 = 1.5 m m o l$ $10xx0.15=1.5mmol$

Explanation:

So the mol ratio is $3.0 \div 1.5 = 2$ $3.0div1.5=2$

Since phosphoric acid does not easily give off its third proton, and if the hydroxide were sodium hydroxide, the most likely equation would be:

$2 N a O H + H_{3} P O_{4} \to N a_{2} H P O_{4} + 2 H_{2} O$ $2NaOH+H_3PO_4->Na_2HPO_4+2H_2O$

Or: $2 O H^{-} (a q) + H_{3} P O_{4} (a q) \to H P O_{4}^{2 -} (a q) + 2 H_{2} O (l)$ $2OH^(-)(aq) +H_3PO_4(aq)->HPO_4^(2-)(aq) +2H_2O(l)$

With (di)sodium (mono)hydrogen phosphate as the resulting salt.

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