Question

Explain(showing each steps in the calculation)you will prepare 1 L of 0.1 M HCL from 1...

Explain(showing each steps in the calculation)you will prepare 1 L of 0.1 M HCL from 1 L of 37% HCL.Molecular weight of HCL is 36.5 g/mol and the density is 1.2 g/ml

Homework Answers

Answer #1

To prepare 1L of 0.1M HCL from 37% HCL we need to first calculate the molarity of 37% HCL.

1. Molarity of 37% HCL :

1.2 g/ml * 1000ml * (0.37/36.5g/mol) = 12.1643 Molar
12 moles of HCL in 1 liter of solution makes 37% HCL

2. Now we can use the formula
M1V1= M2V2
Moles before dilution = Moles after dilution

Required molarity ( M2 )= 0.1M
Required Volume (V2) = 1L = 1000ml
Initial molarity( M1)= 12.1643M
Initail volume (V1) is to be calculated.

Therefore, V1 = M2V2/M1
V1 = 0.1*1000ml/ 12.1643 = 8.22077ml

You should add 8.2207 ml of 37% HCl to make 0.1 M HCL solution

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Aspirin Determination using Back Titration Began with 0.1 M HCl solution and 0.1 M NaOH solution....
Aspirin Determination using Back Titration Began with 0.1 M HCl solution and 0.1 M NaOH solution. 1:2 aspirin to NaOH mole ratio, therefore, mol HCl (back titration) = excess mol NaOH AND total mol NaOH used - excess mol NaOH=required mol NaOH AND required mol NaOH (1 mol aspirin / 2 mol NaOH) = mol aspirin. Each step builds off the last 1) Determination of HCl Concentration. This was the first titration. Concentrated HCl was diluted to .1M before titrating....
a) What volume (to the nearest 0.1 mL) of 6.60-M HCl must be added to 0.450...
a) What volume (to the nearest 0.1 mL) of 6.60-M HCl must be added to 0.450 L of 0.200-M K2HPO4 to prepare a pH = 7.40 buffer? b) How many grams (to the nearest 0.01 g) of NH4Cl (Mm = 53.49 g/mol) must be added to 400. mL of 0.964-M solution of NH3 in order to prepare a pH = 8.75 buffer? pKb = 4.75
You are asked to prepare 1.2 l of a 0.05 M tris buffer at pH= 7.8....
You are asked to prepare 1.2 l of a 0.05 M tris buffer at pH= 7.8. You start with the conjugate base form of tris (121 g/mol). How many grams of tris must you weigh out? How many ml of 6 M HCl (a strong acid) must you add to reach pH=7.8? The pKa for tris is 8.1.
You wish to prepare 100 mL of 0.750 M HCl from concentrated HCl (11.65 M). You...
You wish to prepare 100 mL of 0.750 M HCl from concentrated HCl (11.65 M). You are provided with a 100 mL volumetric flask and a 10 mL graduated pipet with 0.00 line at the top and calibration lines each 0.1 mL. When filled to the 0.00 mL line this pipet would dispense 10.00 mL of solution when drained leaving only the final inside drop. At what volume reading on the pipet should you start dispensing the 11.65 M HCl...
What volume (to the nearest 0.1 mL) of 4.00-M HCl must be added to 0.400 L...
What volume (to the nearest 0.1 mL) of 4.00-M HCl must be added to 0.400 L of 0.150-M K2HPO4 to prepare a pH = 6.50 buffer? mL
What volume (to the nearest 0.1 mL) of 4.70-M HCl must be added to 0.450 L...
What volume (to the nearest 0.1 mL) of 4.70-M HCl must be added to 0.450 L of 0.200-M K2HPO4 to prepare a pH = 7.00 buffer?
Your instructor has asked you to prepare 2.00 L of 0.169 M NaOH from a stock...
Your instructor has asked you to prepare 2.00 L of 0.169 M NaOH from a stock solution of 53.4 (+/- 0.4) wt % NaOH with a density of 1.52 (+/- 0.01) g/mL. (a) How many mL of stock solution will you need? (b) If the uncertainty of delivering NaOH is +/- 0.10 mL, calculate the absolute uncertainty in the molarity (0.169 M). Assume negligible uncertainty in the molecular weight of NaOH and in the final volume, 2.00 L.
Calculate how many milliliters of 1 M NaOH will be needed to make 1 L of...
Calculate how many milliliters of 1 M NaOH will be needed to make 1 L of 0.1 M solution. Calculate how many grams of potassium acid phthalate (KHP, FW = 204.2 g/mol) will react with about 25 ml of the 0.1 M NaOH solution. The reaction is as follows: HKC8H4O4 + NaOH → H2O + NaKC8H4O4 Calculate how many mL of 1 M HCl is needed to make 1 L of 0.2 M HCl. HCl + NaOH → H2O +...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
How would you prepare a .100 L of 50mM succinate buffer at pH 3.85 using solid...
How would you prepare a .100 L of 50mM succinate buffer at pH 3.85 using solid disodium suddinate, DI water and either 1.00 M NaOH or 1.00 M HCL. The formula weight of disodium succiante is 162 g/mol. pka1 = 4.21; pka2 = 5.64.