# If 8.8 mL of an HCl solution is added to water to make 0.300 L of 0.250 M HCl, what was the...

## Question:

If 8.8 mL of an HCl solution is added to water to make 0.300 L of 0.250 M HCl, what was the concentration of the initial HCl?

## Dilution of Solutions:

Solutions are mixtures that are composed of solutes and solvents. New more dilute solutions can be prepared from concentrated stock solutions by adding more solvent. This technique is known as dilution. Dilution does not change the amount of solute present.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerThe given initial and final volume and the given final concentration are listed below.

- {eq} C_1 = ? {/eq}
- {eq} C_2 = 0.250 \ M {/eq}
- {eq} V_1 = 8.8...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 8 / Lesson 5Want to know how to calculate dilution factor? See dilution equations, the dilution formula, and learn how to dilute acid and how to dilute a solution.

#### Related to this Question

- A 112 mL solution of 0.351 M HCl is added to 52.0 mL of 0.161 M HCl. What is the new concentration of HCl?
- You add 3.5 L of an HCl solution of unknown concentration to 2.0 L of 0.5 M HCl and 4.5 L of water. The final concentration of HCl was 1.5 M. What was the unknown concentration of the initial HCl solution?
- How many mL of water must be added to 300 mL of a 0.75 M HCl solution to dilute it to a concentration of 0.25 M?
- If 50 mL of 0.10 M HCl is diluted to a total volume of 100 mL by adding distilled water, what is the HCl concentration in the new solution?
- What volume of water must be added to 30.0 mL of a 0.600 M HCl solution in order to dilute it to a concentration of 0.100 M?
- How much water should be added to 5.0 mL of an 0.080 M HCl solution to dilute it to a concentration of 0.010 M?
- What is the concentration of HCl in the final solution when 65 mL of a 3.0 M HCl solution is diluted with pure water to a total volume of 0.15 L?
- What is the concentration of HCl in the final solution when 65 ml of a 12 m HCl solution is diluted with pure water to a total volume of 0.15 L?
- Water is added to 25.0 mL of a 0.750 M HCI solution until there is exactly 125 mL of solution. What is the concentration of the final solution?
- 500 mL of water is added to 25 mL of 6.0 M hydrochloric acid. What is the final concentration of this solution in mol/L?
- 5.00 mL of 0.0100 M HCl is pipetted into a beaker and diluted with water to 50.0 mL. What is the concentration of HCl?
- What is the concentration when 60.0 mL of a 9.00 M HCl solution is diluted to 1.170 liters?
- 350.0 mL of 2.50 M HCl are added to 400.0 mL of 5.00 M HCl. Assuming that the volumes are additive, what is the final concentration?
- You have 520 mL of a 0.120 M HCl solution and you want to dilute it to a concentration of exactly 0.100 M. How much water should you add?
- A 15.0-mL solution of 12 M HCl is diluted with 200 mL of water. What is the new concentration of the acid solution?
- If 30.00ml of water are added to 20.0 ml of 2.5M HCl solution, what is the resulting diluted molarity?
- What will be the concentration of the solution obtained when 2500 mL of water is added to a 37% v/v 1.19 g/mL (stock bottle) solution of HCl acid?
- Suppose you have 270.0 mL of a 0.125 M HCl solution, and you want to dilute it to a concentration of 0.050 M. How much water should you add?
- If 26.35 mL of 0.2473 M HCl is diluted to 250.0 mL, what is the concentration of the diluted solution?
- A student dilutes 45.0 mL of a 1.67 M HCl solution by adding 80.0 mL of water to total 125 mL. What is the concentration of the diluted HCl solution? a. 2.97 M b. 0.939 M c. 0.601 M d. 1.67 M
- Suppose 85 mL of a 2.0 M HCl solution is diluted with pure water to a total volume of 0.15 L. What is the final concentration of the solution?
- What is the concentration when 54.0 mL of a 6.00 M HCl solution is diluted to 247 milliliters?
- Calculate the volume of concentrated (37 wt.%) HCl that should be added to 500 mL of distilled water to produce a solution with a concentration of 1 M HCl.
- 25.0 ml of 12.0 M HCl are diluted to 500 mL. What is the HCl concentration (molarity) of this dilute solution?
- If 45 mL of 0.25 M HCl is required to completely neutralize 25.0 mL of NH3, what is the concentration of the NH3 solution?
- An aqueous HCl solution with a volume of 40.0 mL is diluted with water to a total volume of 0.765 L. The final concentration of the solution after dilution is 0.15 M. What was the original concentration of the HCl solution before dilution?
- What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by diluting 40 mL of concentrated (11.6 M) HCl to a final volume of 500 mL?
- What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by diluting 15.0 mL of concentrated (11.6 M) HCl to a final volume of 500 mL?
- A 28.9 mL aliquot of a 3.2 M HCl solution is diluted to 454.0 mL of solution. What is the HCl concentration of the diluted solution?
- What volume of water must be added to dilute 5.0 L of .50 M HCl solution into a .10 M solution?
- What is the concentration of each ion present in the solution formed by mixing 50 mL of 0.100 M HCl solution and 10.0 mL of 0.440 M HCl solution?
- A 500 ml bottle of 16 M hydrochloric acid is diluted to a final volume of 5.0 L. What is the concentration of the new diluted, HCl solution?
- If you had a 100 mL of 2.00 M HCl and you added 100 mL to it what is the final volume and final concentration? The volume would be 200ml, but would the concentration just stay the same?
- What is the OH- concentration of a 5 x 10-4 M HCl solution?
- What is the concentration of a solution prepared by diluting 25.0 mL of HCL 0.750 mol/L to a final volume of 500 mL?
- If 50 mL of 0.10 M HCI is diluted to a total volume of 150 mL by adding distilled water, what is the HCI concentration in the new solution?
- To what volume should 16.00 mL of a 11.60 M HCl solution be diluted to prepare a 0.480 M HCl solution?
- if 5.00 ml of 1.66 times 10^{-1} M HCl solution is diluted to exactly 250.0 ml with water, what is the concentration of the resulting solution?
- If 40 mL of 0.50 M HCl is mixed with 60 mL of water, the HCl concentration of the resulting solution will be (blank) M?
- If you wanted to make a 100 L of a 0.1 M solution of HCl(aq), what volume of concentrated 12M HCl would you start with?
- What volume (in mL) of a 1.25 M HCl solution can be made by diluting 75.0 mL of a 12.0 M HCl solution?
- Calculate how many mL of 6 M HCl are needed to prepare 100 mL HCl solution with a concentration of 1 M.
- What volume ml of a concentrated 6.0 m HCl solution is required to prepare 725 ml of .12 m HCl solution?
- If 15.0 mL of 3.0 M HCI are diluted to a final volume of 100.0 mL, what is the new concentration?
- If 56 mL of 1.93 M hydrochloric acid is mixed with water to create a solution with a concentration of 0.9 M, how many liters of water were added?
- 2 ml of 1M HCl 0 ml of H2O 3ml of .3M Na2S2O3 How do I find the initial and final concentrations of both HCl and Na2S2O3?
- To what volume will you have to dilute 30.0 mL of a 12 M HCl solution to make a 0.35 M HCl solution?
- To what volume must 10.0 ml of 5.00 M HCL be diluted to make a 0.500 M HCL solution ?
- Exactly 25.0 mL of 12.0 M HCl is diluted to give a total volume of 250.0 mL. What is the new molarity of the diluted HCl solution? (A) 0.0750 M (B) 0.833 M (C) 521 M (D) 1.20 M
- If 50.00 mL of 1.50 M HCl (aq) is diluted with water to a volume of 1500.0 mL, what is the molarity of the diluted HCl (aq)?
- If 50.0 mL of a 6.00 M HCl stock solution are diluted with water to a final volume of 2.00 L, what will be the final concentration of HCl in the dilute solution? a) 0.0600 M b) 0.600 M c) 0.150 M d) 1.50 M e) 0.300 M f) 3.00 M
- What volume, in L, of a 10.0 M HCl solution is needed to make 2.00 L of 2.00 M HCl solution by dilution with water?
- A scientist wants to make 2.50 L of a 1.50 M HCl solution. The stock HCl solution has a concentration of 12.3 M. What volume of water (in L) will be needed? Assume that volumes are additive.
- If 25.1 mL of a 6.01 M HCl solution is diluted to 1.45 L, what is the concentration (in molarity) of the diluted solution?
- To what volume must 10 ml of 5 M HCl be diluted to make a 0.5 M HCl solution ? A. 1 ml B. 50 ml C. 100 ml D. 500 ml E. 1000 ml.
- To prepare one liter of 2.5 M solution of HCl, what is the volume of concentrated HCl (37% p/p, d = 1.19 g/mL) to be used?
- What is the concentration of HCl in a 250.0 mL sample of hydrochloric acid if 15.5 mL of 0.0100 M NaOH is needed to react with all the HCl?
- If I start with 0.0350 L of a 12.0 M hydrochloric acid solution, and dilute it with water to a new volume of 1.20 L, what is the new concentration?
- During an experiment, 20 ml of 4 M hydrochloric acid is mixed with 30 ml of water. What is the concentration of your new solution?
- If you mix 20 ml of a 6 N HCl with 80 ml of another HCl solution, that resulting mixture has a concentration of 3 N. What is the concentration of the second solution that was used for the mixture?
- What volume of a 0.50 M HCl solution can be prepared from diluting 25 mL of a 2.0 M HCl solution?
- 25.0 ml of HCl reacts with 39.5 ml of 0.150 M K3PO4 solution. 3HCl(aq) + K3PO4(aq) to H3PO4(aq) + 3KCl(aq). What is the concentration of the HCl solution? a) 0.0790 M b) 0.0949 M c) 0.237 M d) 0.711 M
- A 251 mL sample of 0.45 M HCl is added to 455 mL of distilled water. What is the molarity of the final solution? Assume the volumes are additive.
- What is the concentration of H^+ ions in a solution of hydrochloric acid that was prepared by diluting 40 0 mL of concentrated (11.6 M) HCI to a final volume of 500 mL?
- If 20.0 mL of a 0.10 M HCl solution is mixed with 10.0 mL of a 0.25 M HCl solution, what is the final concentration of HCl after the two solutions are mixed?
- What is the final volume after diluting 75.0 mL of a 6.00 M HCl solution to give a 0.200 M HCl solution?
- If 5.00 mL of HCL requires 4.96 mL of 0.958 M NaOH to just consume the HCL, what is the concentration of the HCL?
- 28 mL of 0.10 M HCl is added to 60 mL of 0.10 M Sr(OH)_2. Determine the concentration of OH^- in the resulting solution.
- 2.0 L of a 6.0 M HCl solution is added t owater so that the final volume is 6.0 L. Calculate the new concentration
- 10 mL of a 2.5 M HCl solution was added to 500 mL of 0.20 M HNO_3 solution. What was the concentration of H^+ ion in final solution?
- 25.0 mL of 12.0 M HCl are diluted to 500 mL. HCl is a strong acid. What is the hydrogen ion concentration of this dilute solution?
- What volume of 1.5 M HCl solution do you need to use to make 500 mL of 0.25 M HCl solution by dilution?
- What volume (in mL) of a 12.0 M HCl solution is required to prepare 500 mL of a 0.100 M HCl solution by dilution?
- If 5.00 mL of HCl require 4.59 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
- If 5.00 mL of HCl require 4.03 mL of 0.9581 M NaOH to just consume the HCl, what is the concentration of the HCl?
- What is the concentration of HCl stock solution that can create 250 mL of a 1.0M solution that is prepared by the dilution of 50 mL of the HCl stock solution?
- What volume of 0.149 M HCl must be added to 1.00 times 10^2 mL of 0.285 M HCl so that the resulting solution has a molarity of 0.205 M? Assume that the volumes are additive.
- .1L of a 0.5M soln. of HCl is produced by mixing .25L of HCl stock with water. What's the concentration of stock solution?
- A 0.300 M solution of HCl is prepared by adding some 1.50 m HCl to a 500 ml volumetric flask and diluting to the mark with deionized water. What volume of 1.50 M HCl must be added?
- Starting with a 1.35 M HCl stock solution, five standard solutions are prepared by sequentially diluting 5.00 mL of each solution to 100.0 mL. What is the concentration of the final solution?
- 15% concentrate of HCl (85% water) is mixed with 2 L of water to make a 12% concentrate. What was the initial volume in the mixture?
- If a 25.0 mL sample of 0.500 M HCl solution were diluted 125-fold, what would be the volume and concentration of the diluted solution?
- If 5.0 mL of 0.12 mmol dm-3 MB solution is diluted by adding 20.0 mL of 0.2 mol dm-3 HCl to it, what is the new MB concentration?
- How many mL of a 0.05 M HCl solution can be made by diluting 250 mL of a 5.0 M HCl solution?
- I am 100 mL of a 0.5 M HCl solution, and I want to dilute it to exactly 0.1 M. How much water should I add?
- You have 505 mL of a 0.120 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add?
- You have 505 mL of a 0.175 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add?
- You have 505 mL of a 0.125 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add?
- You have 505 ml of a 0.160 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add?
- What is the concentration of HCl when 25.0 mL of HCl completely reacts with 10.0 mL of 0.1 M solution of NH4OH?
- Calculate the final concentration of the solution when water is added to prepare each of the following solutions. - 30.0 mL of a 11.2 M HCl solution is diluted to 580. mL. - 65.0 mL of a 25.0 %(m/v) NH4Cl solution is diluted to 170 mL. - 9.00 mL of a 9.
- A 35.0 mL sample of an NH3 solution is titrated with a 0.25 M HCl solution. At the endpoint, it is found that 45.0 mL of HCl was used. What was the concentration of the NH3 solution?
- Hydrochloric acid is being diluted with water. If 10.0 ml of 1.78 M acid is used. What is the final concentration if the diluted volume is 215 ml of solution?
- To what volume should you dilute 0.200 L of a 18 M HCl solution to obtain 1.0 M HCl?
- A chemist needs 225 mL of a 2.4 M HCl solution. What volume of a 12.0 M HCl solution must be mixed with water to form this solution?
- Calculate the final concentration of the solution in each of the following situations. 1. Water is added to 0.270 L of a 6.00 M HCl solution to give a volume of 3.00 L. 2. A 31.0 mL sample of a 2.50 M KCl solution is diluted with water to 0.350 L. Expres
- When a solution of 6 M HCl is made from a stock of concentrated HCl by adding an equal volume of water, why is the concentration of the solution only an approximate concentration?
- A 20-ml sample of 5.0 M HCl solution is diluted with water to give 100 mL of solution. The final concentration of the HCl solution is