Calculate the molarity of the following solution from this acid-base titration d

Question

Calculate the molarity of the following solution from this acid-base titration data:

If 100 ml of Ca(OH)2 of unknown concentration with a methyl red indicator present is titrated with [0.350 M] HCl, the yellow solution turns red after 31.8 ml of the HCl is added. What is the molarity of the Ca(OH)2 solution?

Explanation / Answer

Ca(OH)2 + 2 HCl ====> CaCl2 + 2 H2O M1 = molarity of Ca(OH)2 = ? : V1 = volume of Ca(OH)2 = 100mL : n1 = co-efficient of Ca(OH)2 in balanced reaction = 1 M2 = Molarity of HCl = 0.350M : V2 = volume of HCl = 31.8: n2 = co-efficient of HCl in balanced reaction =2 according to titration formula (M1V1/n1) =(M2V2/n2) M1 * 100/1 = (0.350*31.8)/2=5.565 M1 + 5.565/100 = 0.05565 = 0.056 M Ca(OH)2

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