If 112 ml of HCl(g) at STP conditions become the solute in 500ml of water solution, what will be the pH of the mixture

Question

Sakshi · Answer

try to find out the total hydronium ion concentration in order to calculate the pH u also need to refer to the self ionization of water for this question

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If 112 ml of HCl(g) at STP conditions become the solute in 500ml of water solution, what will be the pH of the mixture

If 112 ml of HCl(g) at STP conditions become the solute in 500ml of water solution, what will be the pH of the mixture

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If 112 ml of HCl(g) at STP conditions become the solute in 500ml of water solution, what will be the pH of the mixture

If 112 ml of HCl(g) at STP conditions become the solute in 500ml of water solution, what will be the pH of the mixture

1 Answers

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Other Related Questions on Physical Chemistry

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