Calculate the final concentration of the solution in a 50.0 mL sample of a 2.50 M KCl solution,...
Question:
Calculate the final concentration of the solution in a 50.0 mL sample of a 2.50 M KCl solution, diluted with water to 0.400 L.
The Concentration of Solution:
The concentration of the solution is taken as the total number of moles of the solute that is dissolved in a given amount of solvent. One unit of concentration is molarity. The molarity is computed by getting the ratio of the number of moles of the solute with the total volume of the solution. Higher molarity means a more concentrated solution.
Answer and Explanation: 1
To solve for the final concentration of the KCl, we need to determine first the number of moles present in the 50.0 mL sample.
{eq}\rm moles\,KCl = 2.50\,M \times 0.0500\,L \\ moles\,KCl = 0.125\,moles {/eq}
Now, to solve for the final concentration, we just need to divide the total number of moles by the total volume of the solution.
{eq}\rm [KCl]=\dfrac{0.125\,moles}{(0.0500+0.400)\,L}\\ [KCl]=0.278\,M {/eq}
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Calculating Dilution of Solutions
from
Chapter 8 / Lesson 5
105K
Want 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
- Calculate the final concentration when a 27.0 mL sample of a 4.8% (m/v) KBr solution is diluted with water so that the final volume is 215.5 mL.
- Calculate the final concentration of a 50.0 mL sample of 8.00% (m/v) NaOH that is diluted with water so that the final volume is 200.0 mL.
- Calculate the concentration of a solution if 100 mL of a 2.5 M solution was diluted to 600 mL.
- Calculate the concentration of a solution made by diluting 75.0 mL of 5.3 M HBr to a final volume of 600.0 mL.
- A 5.00 mL sample of an 18.2 M solution is diluted to 0.1100 L. Then 3.00 mL of this solution is diluted to 0.700 L. What is the final concentration?
- What is the final molar concentration after 100-mL of 5.0-M KCl solution is diluted with water to give a final volume of 200-mL?
- If you take an 11.5 mL sample of a 12.6 M NH3 solution and dilute it to a total volume of 0.650 L, what will be the concentration of the final solution?
- What is the final concentration of 35.7 mL of 52.0% m/m solution that is diluted to 65.9 mL?
- You dilute 10.0 mL of a 2.50 M solution to 500 mL. What is the final concentration?
- 75.0 mL of a 1.40 M solution is diluted to a volume of 248 mL. A 124 mL portion of that solution is diluted using 165 mL of water. What is the final concentration?
- 62.0 mL of a 1.70 M solution is diluted to a volume of 288 mL. A 144-mL portion of that solution is diluted using 183 mL of water. What is the final concentration?
- 75.0 mL of a 1.8 M solution is diluted to a volume of 258 mL. A 129-mL portion of that solution is diluted using 187 mL of water. What is the final concentration?
- 72.0 ml of a 1.50 M solution is diluted to a volume of 288 mL. A 144 mL portion of that solution is diluted using 185 mL of water. What is the final concentration?
- 78 mL of a 1.60M solution is diluted to a volume of a 238mL. A 119-mL portion of that solution is diluted using 133 mL of water. What is the final concentration?
- 67.0 mL of a 1.50 M solution is diluted to a volume of 258 mL. A 129 mL portion of that solution is diluted using 163 mL of water. What is the final concentration?
- 7.60 mL of a 1.30 M solution is diluted to a volume of 248 mL. A 124-mL portion of that solution is diluted using 183 mL of water. What is the final concentration?
- 76 mL of 1.40 M solution is diluted to a volume of 288 mL. A 144 mL portion of that solution is diluted using 143 mL of water. What is the final concentration?
- 50.0 mL of a 1.20 M solution is diluted to a volume of 238 mL. A 119-mL portion of that solution is diluted using 141 mL of water. What is the final concentration?
- 75.0 mL of a 1.80 M solution is diluted to a volume of 258 mL. A 129 mL portion of that solution is diluted using 187 mL of water. What is the final concentration?
- What is the final concentration when 25 ml of 0.500 M HCl is diluted to 500 ml with water?
- If 120 mL of a 6 M N a O H solution is diluted to a final volume of 200 mL, what is the resulting concentration of the solution?
- 57.0 mL of a 1.40 M solution is diluted to a total volume of 208 mL. A 104 mL portion of that solution is diluted by adding 105 mL of water. What is the final concentration?
- 54.0 mL of a 1.50 M solution is diluted to a total volume of 258 mL. A 129 mL portion of that solution is diluted by adding 165 mL of water. What is the final concentration?
- A 29.0 g sample of N a O H is dissolved in water, and the solution is diluted to a final volume of 1.60 L. What is the molarity of the final solution?
- If you dilute 17.0 mL of the stock solution to a final volume of 0.330 L, what will be the concentration of the diluted solution?
- If you dilute 18.0 mL of the stock solution to a final volume of 0.290 L, what will be the concentration of the diluted solution?
- If you dilute 18.0 mL of the stock solution to a final volume of 1.00 L, what will be the concentration of the diluted solution?
- If you dilute 21.0 mL of the stock solution to a final volume of 0.500 L, what will be the concentration of the diluted solution?
- If you dilute 10.0 mL of the stock solution to a final volume of 0.350 L, what will be the concentration of the diluted solution?
- If you dilute 18.0 mL of the stock solution to a final volume of 0.270 L, what will be the concentration of the diluted solution?
- If you dilute 15.0 mL of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?
- If you dilute 17.0 ml of the stock solution to a final volume of 0.320 L, what will be the concentration of the diluted solution?
- If you dilute 11.0 mL of the stock solution to a final volume of 0.350 L, what will be the concentration of the diluted solution?
- If you dilute 18.0 ml of the stock solution to a final volume of 0.300 l, what will be the concentration of the diluted solution?
- If you dilute 19.0 mL of the stock solution to a final volume of 0.350 L, what will be the concentration of the diluted solution?
- Calculate the concentration of the final solution, in mol/L. 8.00 � x10^-5 mol was diluted to 500 mL.
- What is the final volume if 10.0 mL of solution with the initial concentration of 0.455 M is diluted to a final concentration of 0.00550 M?
- Calculate the final concentration of the solution in each of the following. (a) Water is added to 10.0 mL of a 3.50 M K N O 3 solution, giving a volume of 0.250 L. (b) A 5.00-mL sample of a 18.0 M sucrose solution is diluted with water to 100. mL. (c
- Calculate the final concentrations of the following aqueous solutions after each has been diluted to a final volume of 25.0 mL. a. 3.00 mL of 0.175M K^+ \\b. 2.50 mL of 10.6 mM LiCl \\c. 15.00 mL of 0.0724 M Zn^{+2} d. The concentration of Cl^- in the
- A 150.0-mL sample of Solution A is diluted to a total volume of 423 mL to form Solution B. If the concentration of Solution A was originally 20.0 mg/L, what is the concentration (in mg/L) of Solution
- If you dilute 20.0 ml of the stock solution to a final volume of 0.320 L, what will be the concentration of the diluted solution?
- If you dilute 14.0 ml of the stock solution to a final volume of 0.260 l, what will be the concentration of the diluted solution?
- If you dilute 13.0 ml of the stock solution to a final volume of 0.340 l, what will be the concentration of the diluted solution?
- If you dilute 17.0 mL of the stock solution to a final volume of 0.270 L, what will be the concentration of the diluted solution?
- If you dilute 13.0 mL of the stock solution to a final volume of 0.330 L, what will be the concentration of the diluted solution?
- What is the final volume. In milliliters, when 10 0 mL of each of the following solutions is diluted to provide the given concentration? 11.5%(m/v) HC1 solution to give a 3 50 %(m/v) HC1 solution 4.00
- Calculate the concentration of a new solution made by placing 15.0 mL of 7.70 mol/L solution into 585.0 mL of water.
- 53.0 mL of a 1.60 M solution is diluted to a total volume of 288 mL. A 144-mL portion of that solution is diluted by adding 121 mL of water. What is the final concentration? Assume the volumes are a
- Calculate the new molarity of a 35 mL sample of 0.450 M CaCl2 solution that is diluted with enough water to make 250 mL of solution.
- What is the final concentration of a solution if 15 mL of a 2.4 M solution was diluted to 100 mL and this process was repeated two more times?
- 71.0 mL of a 1.30 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 105 mL of water. What is the final concentration? Assume the volumes are add
- 58.0 mL of a 1.60 M solution is diluted to a total volume of 288 mL. A 144-mL portion of that solution is diluted by adding 173 mL of water. What is the final concentration? Assume the volumes are add
- 59.0 mL of a 1.60 M solution is diluted to a total volume of 268 mL. A 134-mL portion of that solution is diluted by adding 173 mL of water. What is the final concentration? Assume the volumes are add
- 53.0 mL of a 1.20 M solution is diluted to a total volume of 238 mL. A 119-mL portion of that solution is diluted by adding 185 mL of water. What is the final concentration? Assume the volumes are add
- A 63.0 mL of a 1.30 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 173 mL of water. What is the final concentration? Assume the volumes are a
- 59.0 mL of a 1.40 M solution is diluted to a total volume of 206 mL. A 104-ml portion of that solution is diluted by adding 147 mL of water. What is the final concentration? Assume the volumes are add
- 67.0 mL of a 1.60 M solution is diluted to a total volume of 268 mL. A 134-mL portion of that solution is diluted by adding 131 mL of water. What is the final concentration? Assume the volumes are add
- 52.0 mL of a 1.70 M solution is diluted to a total volume of 258 mL. A 129-mL portion of that solution is diluted by adding 109 mL of water. What is the final concentration? Assume the volumes are add
- 53.0 mL of a 1.50 M solution is diluted to a total volume of 258 mL. A 129 mL portion of that solution is diluted by adding 195 mL of water. What is the final concentration? Assume the volumes are add
- 59.0 mL of a 1.40 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 129 mL of water. What is the final concentration? Assume the volumes are add
- 75.0 mL of a 1.20 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 111 mL of water. What is the final concentration? Assume the volumes are add
- 50.0 mL of a 1.50 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 181 mL of water. What is the final concentration? Assume the volumes are add
- 75.0 mL of a 1.40 M solution is diluted to a total volume of 228 mL. A 114-mL portion of that solution is diluted by adding 159 mL of water. What is the final concentration? Assume the volumes are add
- 74.0 mL of a 1.30 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 151 mL of water. What is the final concentration? Assume the volumes are add
- 54.0 mL of a 1.40 M solution is diluted to a total volume of 208 mL. A 104-mL portion of that solution is diluted by adding 109 mL of water. What is the final concentration? Assume the volumes are add
- 59.0 mL of a 1.60 M solution is diluted to a total volume of 268 mL. A 134-mL portion of that solution is diluted by adding 111 mL of water. What is the final concentration? Assume the volumes are add
- 54.0 mL of a 1.30 M solution is diluted to a total volume of 258 mL. A 129-mL portion of that solution is diluted by adding 147 mL of water. What is the final concentration? Assume the volumes are add
- 61.0 mL of a 1.30 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 129 mL of water. What is the final concentration? Assume the volumes are add
- 69.0 mL of a 1.80 M solution is diluted to a total volume of 258 mL. A 129 mL portion of that solution is diluted by adding 109 mL of water. What is the final concentration? Assume the volumes are add
- 52.0 mL of a 1.50 M solution is diluted to a total volume of 288 mL. A 144-mL portion of that solution is diluted by adding 189 mL of water. What is the final concentration? Assume the volumes are add
- 77.0 mL of a 1.20 M solution is diluted to a total volume of 288 mL. A 144 mL portion of that solution is diluted by adding 155 mL of water. What is the final concentration? Assume the volumes are add
- 75.0 mL of a 1.50 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 139 mL of water. What is the final concentration? Assume the volumes are add
- 52.0 mL of a 1.50 M solution is diluted to a total volume of 208 mL. A 104-mL portion of that solution is diluted by adding 147 mL of water. What is the final concentration? Assume the volumes are add
- 59.0 mL of a 1.20 M solution is diluted to a total volume of 218 mL. A 109-mL portion of that solution is diluted by adding 147 mL of water. What is the final concentration? Assume the volumes are add
- 50.0 mL Of a 1.40 M solution is diluted to a total volume of 218 mL. A 109-mL portion of that solution is diluted by adding 121 mL of water. What is the final concentration? Assume the volumes are add
- 64 0 mL of a 130 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 163 mL of water. What is the final concentration? Assume the volumes are addi
- 65 0 ml of a 1.40 M solution is diluted to a total volume of 238 mL. A 119-mL portion of that solution is diluted by adding 187 mL of water. What is the final concentration? Assume the volumes are add
- If 5.0 mL of a 1.25 M solution is diluted to 25.0 mL, what is the final molarity of the dilute 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
- Determine the concentration of a solution made by adding 10.0 mL of 10.0 mol/L acid to 600.0 mL of water.
- What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L? A) 0.0167 B) 1.67 C) 3.0 D) 0.600
- What is the concentration of a solution made by diluting 45 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 95 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 15 mL of 6.0 M HCI to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 85 mL of 6.0 M HCI to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 35 mL of 6.0 M HCI to a final volume of 750 mL? ................ M
- What is the concentration of a solution made by diluting 75 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 65 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 35 ml of 6.0 M HCL to a final volume of 750 ml?
- What is the concentration of a solution made by diluting 25 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 55 ml of 6.0 M HCl to a final volume of 750 ml?
- If 43.6 mL of 6.00 M solution is diluted to 250.0 mL, what is the final molarity of the solution?
- (a) A 25.0-mL sample of HCl(aq) is diluted to a volume of 500.0 mL. If the concentration of the diluted solution is found to be 0.085 M HCl, what was the concentration of the original solution? (b) A
- A 2.0 L of a 1.5 M solution is diluted with water until the final volume is 6.0 L. The molarity of the solution is now _____.
- If 4.00 mL of a stock solution is diluted to 5.00 mL, what is the concentration of the final solution relative to the concentration of the stock solution?
- If you have a solution that is 0.50 mol/L, and you then take 35 mL of this solution and make it up to 175 mL total volume by diluting it with water, what is the new concentration?
- If water is added to 50 mL of a 0.04 M solution so that it fills a 200 mL beaker, what is the final concentration?
- 15.0 mL of a 0.95 M Cu^{2+} solution was diluted with H_2O to a total volume of 26.0 mL. What is the molar concentration of Cu^{2+} in the diluted solution?
Explore our homework questions and answers library
Browse
by subject