molarity of HCL solution?

Question

what is the molarity of an HCL solution of 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?

Answer 1

.4 M x .04L = .016 mole of Base .. = Mole of Acid

.016mol/ .05 = .32 Molarity HCL

Learn to do this... confusing at first, but once u get it, it is a piece of cake..
Learn: mole of acid = mole of base only at equiv point, therefore when it finish titrate, u know how much mole u have (for base), u will realize that mole of acid is the same... just divide that by the volume of acid = molarity.

Answer 2

remember the equation for Molarity? Molarity = 1mol/Liter of answer so because you've 4.82mL/1000 with the point to transform to Liters = .00482L and than different that by the Molarity( of naoh) to get the moles of NaOH = ( 00482L) (0.262 M) =.00126moles because the HCL and NaOH are in a a million:a million ratio the moles of Hcl is an similar with that of NaOH to calculate Molarity of HCl plug the moles and the volume interior the Molarity equation and reember to to transform to Liters so M = .00126moles/ ( .00479L) = .263M

Answer 3

You used 0.04 L of the NaOH solution, which was 0.4 mol/L, so you used a total of 0.4*0.04 = 0.016 mol NaOH. It takes one mole of NaOH to neutralize a mole of HCl, so you neutralized 0.016 moles of HCl. The solution was 0.05 L, so the molarity was 0.016 mol/0.05 L or 0.32 M. This passes the common-sense check because it took a little more HCl solution than NaOH solution, so it makes sense that the HCl solution is a little more dilute.

Answer: 0.32 M