please help, i cannot figure out where i went wrong! Constants Periodic Table Yo
ID: 576199 • Letter: P
Question
please help, i cannot figure out where i went wrong!
Constants Periodic Table You may want to reference Section 13.5 while completing this problem. concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mI PartA How much concentrated solution would it take to prepare 2.70 L of 0.445 M HCl upon dilution with water? v- 94.028 mL Submit Ans Ans X Incorrect; One attempt remaining: Try Again; no points deducted Not quite. Check through your calculations; you may have made a rounding error or used the wrong number of significant figures. Provide Feedback Next>Explanation / Answer
1st find the concentration of concentrated solution
Let volume of solution be 1 L
volume , V = 1 L
= 1*10^3 mL
density, d = 1.2 g/mL
use:
mass = density * volume
= 1.2 g/mL *1*10^3 mL
= 1200.0 g
This is mass of solution
mass of HCl = 37.0 % of mass of solution
= 37.0*1200.0/100
= 444.0 g
Molar mass of HCl,
MM = 1*MM(H) + 1*MM(Cl)
= 1*1.008 + 1*35.45
= 36.458 g/mol
mass(HCl)= 444.0 g
use:
number of mol of HCl,
n = mass of HCl/molar mass of HCl
=(444.0 g)/(36.458 g/mol)
= 12.18 mol
volume , V = 1 L
use:
Molarity,
M = number of mol / volume in L
= 12.18/1
= 12.18 M
use dilution formula
M1*V1 = M2*V2
1---> is for stock solution
2---> is for diluted solution
Given:
M1 = 12.18 M
M2 = 0.445 M
V2 = 2.70 L
use:
M1*V1 = M2*V2
V1 = (M2 * V2) / M1
V1 = (0.445*2.70)/12.18
V1 = 0.0986 L
V1 = 98.6 mL
Answer: 98.6 mL