20 mL of a 0.125 M HCl solution were neutralised by 25 mL of a KOH solution. The equation for the reaction is HCl(aq) + KOH(aq)  KCl(aq) + H2O(l) (not balanced) (a) How many moles of HCl were consumed? How many moles of KOH were neutralised? (c) How many moles of KOH were there in 25 mL of the KOH solution? (d) Calculate the concentration in mol/L of the KOH solution. solution.

20 mL of a 0.125 M HCl solution were neutralised by 25 mL of a KOH sol

1.	20 mL of a 0.125 M HCl solution were neutralised by 25 mL of a KOH solution. The equation for the reaction is HCl(aq) + KOH(aq)  KCl(aq) + H2O(l) (not balanced) (a) How many moles of HCl were consumed? How many moles of KOH were neutralised? (c) How many moles of KOH were there in 25 mL of the KOH solution? (d) Calculate the concentration in mol/L of the KOH solution. solution.
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