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Calculate the pH of a 0.01 M HCl solution.
HCl is a strong electrolytes and thus its complete dissociation will produce a solution O.O1 M (10-2 M) in H+. Since the concentration of H+ arising from water dissociation (10-7 M) is notably lesser than 10-2 M, it can be neglected and thus
pH = -Log (10-2) = 2
HCl is a strong electrolytes and thus its complete dissociation will produce a solution O.O1 M (10-2 M) in H+. Since the concentration of H+ arising from water dissociation (10-7 M) is notably lesser than 10-2 M, it can be neglected and thus
pH = -Log (10-2) = 2
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okk
Calculate the pH of a 0.01 M HCl solution.
HCl is a strong electrolytes and thus its complete dissociation will produce a solution O.O1 M (10-2 M) in H+. Since the concentration of H+ arising from water dissociation (10-7 M) is notably lesser than 10-2 M, it can be neglected and thus
pH = -Log (10-2) = 2
HCl is a strong electrolytes and thus its complete dissociation will produce a solution O.O1 M (10-2 M) in H+. Since the concentration of H+ arising from water dissociation (10-7 M) is notably lesser than 10-2 M, it can be neglected and thus
pH = -Log (10-2) = 2
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