A question about molarity. - Tilted Forum Project Discussion Community

roadkill · 04-05-2007, 12:20 PM

I just started thermodynamics, and I seem to have forgotten some of my basic molarity knowledge.

Given Information.
Equation: HCl + NaOH -> NACL + H20

Vol HCl and NaOH = 50mL or .05L

Molarity HCl and NaOH = 2M

I calculated that I have .1mol of both. Thus there is no remainder.
But I'm suppose to calculate the products.

My question is that if I have .1mol HCL does that mean I have .1mol H and .1mol Cl or do I need to divide the amount in half because it's .1mol total?

Thanks.

n0nsensical · 04-05-2007, 07:21 PM

.1 mol HCl means you have .1 mol of both H+ and Cl- (because 1 HCl molecule dissociates into 1 H+ ion and 1 Cl- ion). You also have .1 mol Na+ and OH-. The products are .1 mol H2O and .1 mol NaCl.

04-05-2007, 12:20 PM	#1 (permalink)
roadkill Insane	A question about molarity. I just started thermodynamics, and I seem to have forgotten some of my basic molarity knowledge. Given Information. Equation: HCl + NaOH -> NACL + H20 Vol HCl and NaOH = 50mL or .05L Molarity HCl and NaOH = 2M I calculated that I have .1mol of both. Thus there is no remainder. But I'm suppose to calculate the products. My question is that if I have .1mol HCL does that mean I have .1mol H and .1mol Cl or do I need to divide the amount in half because it's .1mol total? Thanks.

04-05-2007, 07:21 PM	#2 (permalink)
n0nsensical Junkie Location: San Francisco	.1 mol HCl means you have .1 mol of both H+ and Cl- (because 1 HCl molecule dissociates into 1 H+ ion and 1 Cl- ion). You also have .1 mol Na+ and OH-. The products are .1 mol H2O and .1 mol NaCl. Last edited by n0nsensical; 04-05-2007 at 07:24 PM..