Question

200ml of 1M HCL is mixed with 300ml of 6M HCL & the final solution is diluted to 1000ml.
Calculate molar concentration of \[[H^+]\] ion.

Answer 1

1M HCl => 1 L of solution contains 1 mole of HCl i.e. 1 mole of H+ ions.

moles of H+ ions in 200ml of 1M HCl = 0.2 (1L contains 1 mole so 200 ml contains ? )

moles of H+ ions in 300ml of 6M HCl = 0.3*6 (6M => 6 moles of ions in 1 L solution)

Total moles of H+ ions = 0.2+0.18 = 0.38
Final volume of solution = 1L
So, final concentration of H+ = 0.38/1 = 0.38M

Answer 2

but @FoolAroundMath answer is 2M.

Answer 3

i got your answer:
V1=0,2 dm3
c1=1M
V2=0,3 dm3
c2=6M
V3= V1+V2 = 0,5 dm3

c1V1+c2V2=c3V3
c3= (c1V1+c2V2)/V3
c3= 1*0,2 + 6*0,3 /0,5
c3= 4M

now lets make it simple and say c3 is new c1
c1= 4M
V1= 0,5 dm3
V2=1 dm3

c1V1=c2V2
c2= c1V1/V2
c2= 4*0,5 / 1 = 2M

Answer 4

So @Kryten u mean that final concentration of solution is same as molar concentration of H+ ions ??????????????????

Answer 5

because HCl is strong acid we take that it completly dissociates in water/solution and yes [H+] is equal to concentration of HCL.

Answer 6

oh thanx a lot:)

Answer 7

oh yeah .. my bad 3*0.6 = 0.18 ... good job me . rofl
and yes it is 2M

Answer 8

3*0.6 = 1.8
total moles of H+ = 0.2+1.8 = 2
=> concentration = 2/1 = 2M

Answer 9

oh u r correct too :)
I only observed ur answer
sorry.