Question

In each of the following acid-base reactions, 25.0mL of an HCl solution (the acid) completely reacts 10.0mL of a 0.100M solution of the second reactant (the base). Calculate the concentration of the HCl solution in each case.

4HCl(aq) + NaAl(OH)4(aq) --> AlCl3(aq) + 4H2)(l) + NaCl(aq)

Please show me step by step. Thank You

Answer 1

@apoorvk

Answer 2

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Answer 3

Completely reacts means the mole ratio will exactly match the coefficient ratio of the reactants and products in the balanced reaction (no leftovers). So, in this first reaction, there will be 4x moles of acid (HCl) compared to base (NaAl(OH)4).

Moles of base = volume (L) x concentration (moles/L) = (0.0100 L) x (0.100 M) = 0.00100 moles.

So, moles of acid should be 4 x (0.00100) = 0.00400
There is 0.0250 L of HCl, so the concentration (moles/L) = 0.00400 moles / 0.0250 L = 0.160 M