Dilution Calculations

Key Questions

• How does dilution affect the reaction rate?

  Answer:

  The more the solution of a reactant is diluted, the slower the reaction will occur.

  Explanation:

  The key thing you need to understand here is that chemical reactions depend on reactant particles bumping into each other (collision theory).

  The more concentrated a reactant is, the more likely it will be to bump into other reactants and product chemical change.

  Here is video of a quick lab performed to test this. In the video, varying concentrations of #Na_2S_2O_3# are allowed to react with HCl. A timer is included in the video so you can see how the changing concentration changes the overall speed of the reaction!

  
  video from: Noel Pauller

  Hope this helps!

  mrpauller.weebly.com · 15 · Jan 28 2015

• How do you calculate concentration from absorbance?
• How do you calculate concentration from titration?
• How do you calculate dilution factor?
• How do you calculate serial dilutions?
• How to calculate concentration of solution when it's diluted?
• What are some examples of dilution calculations?
• What would be the concentration of a solution made by adding 250 mL of water to 45.0 mL of 4.2 M KOH?
• What would be the concentration of a solution made by diluting 45.0 mL of 4.2 M KOH to 250 mL?
• What is the molarity of a solution that is made by diluting 50.00 mL of a 4.74 M solution of HCl to 250.00 mL?
• What volume of water would you add to 15.00 mL of a 6.77 M solution of nitric acid in order to get a 1.50 M solution?
• What volume of water would be added to 16.5 mL of a 0.0813 M solution of sodium borate in order to get a 0.0200 M solution?
• How can I calculate the dilution factor using concentration?
• Commercially available concentrated sulfuric acid is 18.0 M H2SO4. What volume of concentrated H2SO4 would I use in order to make 3.00 L of a 4.0 M stock solution?
• Phosphoric acid is commonly supplied as an 85% solution. What mass of this solution would be required to prepare 600.0 mL of a 2.80 M phosphoric acid solution?
• How can I calculate dilution concentration?
• How does dilution affect the pH of a basic solution?
• How does dilution affect the reaction rate?
• How does dilution affect molarity?
• How does dilution affect equilibrium?
• How does dilution affect conductivity?
• How does dilution affect concentration?
• How does dilution affect absorbance?
• How do you do dilution calculations?
• How would you prepare 1.0 L of a 0.10 M solution of sulfuric acid from a 3.0 M solution of sulfuric acid?
• A stock solution contains 51.24 g of barium hydroxide in 1.20 L of solution. How do I make 1.00 L of 0.100 mol/L barium hydroxide from the stock solution?
• What volume of diluent must I add to 1 mL of a 4 mg/L solution of dexamethasone to get a concentration of 2.5 mg/L? Bonus: What volume of the diluted solution contains 0.35 mg of dexamethasone?
• Question #2766f
• Question #e4ec1
• Question #e0588
• Question #9c6e6
• Question #a6138
• Question #77da8
• Question #eed53
• Question #1a210
• Question #1741d
• Question #dfb12
• Question #269be
• Question #4cfc3
• Question #ec0eb
• Question #a18e4
• Question #104c1
• Question #140c8
• Question #1a2db
• You prepare 3.00 L of 0.250 M HNO3 from a stock of nitric acid that is 12.0 M. What volume of the stock solution will you require to make the dilute solution? a) 0.0625 mL b) 62.5 L c) 144 L d) 62.5 mL
• Question #898c4
• How could I prepare a 1 ppm solution of ammonium chloride in water?
• Question #82b49
• Question #80880
• Question #8bd13
• What is the molarity of an H2SO4 solution if 18.5 mL of 0.18 M NaOH are needed to neutralize 25.0 mL of the sample? H2SO4 + 2NaOH => Na2SO4 + 2H2O
• Question #d5ccd
• If 500ml of Lanthnum Chloride solution is enough to remove 1ppm PO4 from 1000L of water, what effect would a dosage of 166ml have on a volume of 30L?
• For example, i am given a problem, how do ik if it' a diluton problem. I know that for dilution the concentration decreases and the volume increases?
• Question #ca68c
• Question #cf103
• Question #5f140
• Question #16d0c
• Question #e73b2
• How would you prepare a 0.2 M #NaOH# solution with a volume of 200 ml, from a 0.12 M #NaOH# solution with a volume of 200 ml?
• Numerical: How will you make a 0.35 M glucose solution? Also, prepare a 0.12 M solution of glucose from the above stock.
• Can you help me? From a 0.5 M #Na_2CO_3# solution having a volume of 300 ml, prepare a 0.075 M #Na_2CO_3# solution with a volume of 150 ml.
• It is desired to prepare 4.0 M nitric acid from the available acid solution of strength 1.4 M & 6.8 M respectively. If the total volume of the 4.0 M nitric acid required to be prepared is 4 #dm^3#, calculate the volume of the 2 acid solutions to be mixed?
• How do we dilute a bacterial culture 50-fold, 100-fold, and 200-fold?
• Question #64184
• Question #a24ac
• Question #e7667
• Question #dfd4e
• Question #e01b7
• Question #c5ab5
• Question #689e9
• Question #cfc54
• Question #63a58
• Question #0c0b4
• What is the percentage concentration by mass of a #16*mol*L^-1# solution of nitric acid, for which density is #1.42*g*mL^-1#?
• Question #47a1f
• Question #59098
• Question #80d6a
• Question #59aee
• How would you prepare 250 mL of 0.158 M solution of #MgCl_2# from a 3.15 M stock solution?
• What is the concentration of a solution formed by diluting 190 mL of 18 M HCL solution to 730 mL?
• Question #2e118
• What volume of 12 M HCl is needed to make 500 mL of .10 M HCl?
• Question #17e71
• Question #1037e
• Question #41e95
• Question #91f35
• How many milliliters of sulfuric acid is required to make an aqueous solution with a pH of 6 if the solution is 0.065 L from a bottle of 12M sulfuric acid?
• Question #55f68
• Question #fc073
• You want to produce 579 mL of a 0.440 M solution of NaCl. You have a 1.40 M solution. How many mL of it should you use and dilute with water?
• What is the final concentration of a solution prepared by adding water to 50.0 mL of 1.5 M NaOH to make 1.00 L of solution?
• Question #b8448
• In a serial dilution, 0.1 mL of serum is added to 1.9 mL of saline in the first tube. The next tubes contain 1.5 mL of saline, and 0.5 mL from the previous tube is added to the next tube. How do we calculate dilution in the next tubes?
• Question #f5c04
• Question #cbbe3
• Question #cbe8e
• What volume of 0.25 M #HCl# solution must be diluted to prepare 1.00 L of 0.040 M #HCl#?
• How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
• Question #a3b28
• Question #03711
• Question #071e7
• Question #457e2
• Question #d755f
• To 225 mL of a 0.80M solution of #KI#, a student adds enough water to make 1.0 L of a more dilute #KI# solution. What is the molarity of the new solution?
• Suppose you have 125.0 mL of 0.400 M #NaCl# solution. This is too salty, so you dilute it by adding another 50.0 mL of water. What is the new concentration of #NaCl# in units of molarity?
• How many milliliters of a solution of 4.00M #KI# are needed to prepare 250.0 mL of 0.760M #KI#?
• 25 mL of a #"10% m/v"# #NH_4Cl# solution is diluted to 250 mL. What is the final concentration of the #NH_4Cl#?
• Question #c5d21
• How do we describe the solution behaviour of #PbCl_2(aq)#?
• Question #0c5a9
• If 30.0 mL of 12.0 M #HCl# stock solution are diluted to a volume of 500 mL, what is the molarity of the dilute solution?
• Question #8f49b
• Question #a14ed
• What is the molarity of a stock solution if 10 mL is diluted to 400 mL with a concentration of 0.5M?
• Question #12ca1
• How many milliliters of 12.0 M #HCl(aq)# must be diluted with water to make exactly 500. mL of 3.00 M hydrochloric acid?
• What is the final volume when 2.50 mL of a 11.0 M #HCl# solution is diluted to 0.100 M #HCl# solution?
• Question #69a7c
• Question #70738
• To what volume should you dilute 55 mL of a 11 M stock #HNO_3# solution to obtain a 0.137 M #HNO_3# solution?
• Given a 2.2 M #MgCl_2# stock solution, how much stock solution (in mL) would be necessary to prepare 250 mL of aqueous 0.115 M #MgCl_2#?
• 800. mL of solution has a concentration of 3.0 M. How much water needs to be added to dilute the solution to 1.9 M?
• A solution was prepared by dissolving 66.6 g of calcium chloride in enough water to make 175 mL of solution. This solution was then further diluted to a total of 550 mL with water. What was the concentration of the final solution?
• Question #b28e9
• 375mL of a 0.455M sodium chloride (#NaCl#) solution is diluted with 1.88L of water. What is the new concentration in molarity?
• What volume (in L) of a 4.13 M lithium nitrate #LiNO_3# solution would be needed to make 195 mL of a 1.05 M solution by dilution?
• What volume (in L) of a 2.46 M magnesium nitrate #Mg(NO_3)_2# solution would be needed to make 275 mL of a 0.758 M solution by dilution?
• What volume (in L) of a 3.95 M potassium chloride, #KCl#, solution would be needed to make 325 mL of a 2.76 M solution by dilution?
• What volume of 0.10 M #NaOH# can be prepared from 250 mL of 0.30 M #NaOH#?
• Question #e11f9
• What is the concentration of a solution prepared by diluting 20.0 mL of a .200 M #NaCl# to 250.0 mL?
• To make 500 mL of 3.0 M #HCl#, how many liters of concentrated 18.0 M #HCl# does one need?
• What volume of 5.0 M #NaOH# is required to make 100 mL 2.0 M #NaOH#?
• If I have 340 mL of a 0.5 M #NaBr# solution, what will the concentration be if l add 560 mL more water to it?
• Question #3678d
• Question #6e951
• How many liters of 8.0M #HCl# are needed to prepare 1.50 L of 2.5M #HCl#?
• Question #23bd9
• A 0.500 L solution of 6 M #HCl# has to be made. How much 12 M #HCl# is needed?
• If 250.0 mL of a 0.96 M solution of acetic acid (#C_2H_4O_2#) are diluted to 800.0 mL, what will be the approximate molarity of the final solution?
• Question #f685a
• Question #ab266
• Question #f8b78
• How do I make 100 ml of .3 M HCl from 1 M?
• What is the final concentration of 50.0 mL of a 2.00M solution, diluted to 500.0 mL?
• How many milliliters of 12.0 M #HCl# (aq) are needed to prepare 215.0 mL of 1.00 M #HCl# (aq)?
• Question #f9869
• What volume of 0.0500M KOH solution is required to completely neutralize 3.0 mL of 0.17M H2SO4?
• Question #3e3f6
• How many milliliters of 12.0 M hydrochloric acid (#HCl#) is required to prepare 0.75 L of a 0.25 M solution of #HCl#?
• 300 mL of water is added to 5 mL of a 12 M solution of #"KI"#. What is the resulting molarity of the solution?
• What is the volume, in mL, of a 2.50M #HCl# solution that must be used in order to create a 350 mL 1.15M #HCl# solution?
• Question #2b75e
• A .50 M solution of sodium thiosulfate, #Na_2S_2O_3#, is used to create a more dilute solution. If 250 mL of the concentrated solution is diluted to a volume of 2.5 L, determine the concentration of the new solution?
• How much 0.12 M #HNO_3# solution can be made by diluting 250 mL of 3.4 M #HNO_3#?
• What volume of concentrated hydrochloric acid (12.0 M #HCl#) is require to make 2.0 liters of a 3.0 M #HCl# solution?
• What volume of a 6.0 M #HCl# solution is required to make 250.0 milliliters of a 1.5 M #HCl#?
• If a student needs to make exactly 2.5 liters of a 1.25 M solution of acetic acid from the 12.0 M stock solution in the chemistry closet, what volume of the stock solution should be used?
• What volume (in mL) of a 3.50M #LiF# stock solution would you use to make 1.5L of 0.500M #LiF# solution?
• What volume of 4.00 M #H_2SO_4# is needed to prepare 500.0 mL of a solution that is 0.850 M in #H_2SO_4#?
• 358ml of an H3PO4 solution is completely titrated by 876mL of 0.0102M Ba(OH)2 solution?
• Is #"Ba"("OH")_2 + "H"_3"PO"_4 -> "BaHPO"_4 + 2"H"_2"O"# a possible reaction?
• Calculate the molarity of H3Po4 if 358ml of H3PO4 solution is completely titrated by 876ml of 0.0102M Ba(OH)2 solution? 2H3PO4+3Ba(OH)2= Ba3(PO4)2 +6H2O?
• What volume of a 6.84M sodium bromide solution would be needed to make 588mL of a 1.84M solution by dilution?
• Question #ba256
• A lab assistant needs to make up 6.00 liters of .100 M HCI solution. How many liters of 12.0 M HCl solution should she use?
• Question #45e44
• A chemistry teacher adds 50.0 mL of 1.50 M #H_2SO_4# solution to 200 mL of water. What is the concentration of the final solution?
• Question #9176b
• 58.0 mL of a 1.30 M solution is diluted to a total volume 248 mL. A 124-mL portion of that solution is diluted by adding 165 mL of water. What is the final concentration? Assume the volumes are additive
• Question #a1f1a
• What is the dilution factor if a 200 µL sample is diluted by adding 500 µL and then 300 µL of solvent?
• What is the threshold odor number (TON) for the follow- ing sample?
• What volume of 3.0 M #HNO_3 (aq)# must be diluted to make 4.0 L of 0.20 M #HNO_3(aq)#?
• Question #67370
• Question #2a118
• What is the molar concentration of the solution after adding 1 mL of 6.00 mol/L #"HCl"# to 499 mL of water?
• Question #e0941
• If somehow, #"50.0 mL"# of a stock solution of #"120. M"# #"HCl"# is available, what volume of water should the appropriate amount of #"HCl"# be added to, in order to reduce its concentration to #"4.00 M"#?
• To what volume should you dilute 20 mL of a 12 M #H_2SO_4# solution to obtain a 0.16 M #H_2SO_4# solution?
• Question #3e0d5
• Question #2a04f
• Concerning the 10.0 mL of 0.50 M NaCl diluted to 100 mL of solution: when a solution is diluted, does the dilution change the number of grams dissolved?
• After performing a dilution calculation, you determine you need 25.0 milliliters of an aqueous stock solution to make 100.0 milliliters of a new solution. How would this be prepared?
• A #295*mL# volume of solution that is #1.00*mol*L^-1# with respect to #"ammonium chloride"# is diluted with a #2.25*L# volume of fresh solvent. What is the resultant #[NH_4Cl]#?
• Question #4ab7b
• Question #0a1c0
• How is moles the same in dilution?
• Question #992dd
• Question #96ad4
• Question #a9870
• Question #183d5
• Question #93cfa
• What volume of water must be added to #57*mL# of #0.500*mol*L^-1# solution to make #285*mL# of #0.100*mol*L^-1# solution?
• Question #8edc0
• Question #6a10d
• Question #c541c
• What volume of #0.200*mol*L^-1# of #NaOH(aq)# would react with a mass of #0.5466*g# of #"KHP"#?
• Question #19c82
• Question #2ade7
• What mass of potassium chloride should be dissolved in a #500*mL# volume of aqueous solution to give a concentration of #1*mol*L^-1#?
• Question #64952
• Does addition of distilled water to an acid-base titration affect the end-result?
• What volume of #12*mol*L^-1# #NaOH# is required to make a #1*L# volume of #4*mol*L^-1# concentration?
• What mass of sodium hydroxide is required for a #1*L# volume of #3*mol*L^-1# sodium hydroxide solution?
• You have 67.0 mL of a 0.400 M stock solution that must be diluted to 0.100 M. Assuming the volumes are additive, how much water should you add?
• What volume of water should be added to 500 mL of a 1.0 mol/L #CuSO_4# (aq) solution to dilute it to 0.5 mol/L?
• Question #780de
• Question #682c7
• Question #a8e62
• What is the resultant concentration when a #30*mL# of a #2.0*mol*L^-1# are diluted to a new volume of #150*mL#?
• A 1.59-g sample of a metal chloride, #MCl_2#, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. How do you calculate the molar mass of M?
• How do you perform a serial dilution?
• Question #d3141
• Do the units used to express the volume of the solution affect the dilution factor?
• How do we use the #"Beer-Lambert law"# to assess concentration?
• Roman mixes 12 litres of 8% acid solution with a 20% acid solution, which results in a 16% acid solution. How do you find the number of litres of 20% acid solution in the new mixture?
• How many milliliters of water must be added to 300 ml of 70% alcoholic solution to make a 40% alcoholic solution?
• Question #ff032
• Question #76612
• Question #708f5
• What is meant by a #"dilute solution"#?
• Question #06a7b
• Question #617c9
• Question #421fb
• A #75*mL# volume of #3.80*mol*L^-1# #"iron(II) sulfate"# is diluted to #4.0*L#. What is the new concentration?
• Question #56faa
• Question #7fc93
• To what volume must a #250*mL# volume of #10*mol*L^-1# #HCl# be diluted to give a #0.050*mol*L^-1# concentration?
• Question #106e8
• Question #85697
• Question #53829
• Question #7b64f
• #"750. mL"# of a #"5.0 M"# solution needs to be diluted to #"1.0 M"#. How much water should be added to reach this concentration?
• What volume OF SOLVENT must we add to a #500*mL# solution of #1.2*mol*L^-1# concentration to dilute the concentration to #1.0*mol*L^-1#?
• To what volume must 440.0 mL of 3.50 M #KNO_3# be diluted to produce 1.50 M #KNO_3#?
• What is #"concentration"#? How does concentration change when volume changes?
• Question #f3cad
• Question #ba6e5
• Question #f8a59
• What is the concentration of a #10*cm^3# volume of a #H_2O_4# at #9.8*mol*dm^-3# concentration that is diluted to a #100*cm^3# volume?
• Question #27266
• Question #6a996
• How much of 8.00 mol/L sulphuric acid must you add to an empty 750. mL bottle to obtain a concentration of 1.50 mol/L?
• What volume of 133 mL, 7.90 M #CuCl_2# solution should you dilute in order to have 51.5 mL of diluted solution that contains 4.49 g #CuCl_2#?
• What is the concentration of a sulphuric acid solution if 25.0 mL of the 36.0% w/v acid is taken by pipette and added to 500. mL of water?
• Question #717a6
• A #75*mL# volume of #0.211*mol*L^-1# #NaOH# was diluted to #125*mL#. What is the new concentration?
• Question #440a6
• Question #9cb3f
• What is the new concentration of a #50*mL# volume of #3.3*mol*L^-1# #HCl(aq)# that is diluted to a #350*mL# volume with fresh water solvent?
• Question #fba72
• A #0.25*L# volume of #0.010*mol*L^-1# concentration was obtained by diluting a WHAT volume of a mother solution of #0.50*mol*L^-1# concentrations?
• How do you mix concentrated acid with water?
• Question #9cf86
• Question #4fac8
• Should we add a base to water, or do the reverse?
• Question #216ab
• How do you make a 1/50 dilution?
• Question #91c2b
• Question #2af68
• If #"250 mL"# of water is added to #"45.0 mL"# of a #"4.2 M KOH"# solution, what will be the final concentration?
• Question #9d93c
• A 15.00 mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 x 10^3 mL. The concentration of the final solution is 0.00383 M. What is the molarity of the original solution?
• Question #1f9b2
• What is the molarity of the solution prepared when #13.50*mL# of #8.00*mol*L^-1# #"hydrochloric acid"# is add to #225.0*mL# of water?
• What volume of distilled water must we add to 50 mL of a 20 % solution to get concentrations of 15 %, 10 % and 5 %?
• Question #bce3f
• How do you solve dilution problems in chemistry? For example: if 211 mL of water is added to 5.00 mL of 3.24 M NaCl solution, what is the concentration of the dilute solution? ____ M.
• You have a microtube containing 1 mL of a solution with #4.3 x 10^4# cells/mL and you are to produce a solution that contains 43 cells/mL. What dilutions must you perform?
• Question #e36df
• A 1/8 dilution of the stock solution is made followed by a 1/6 dilution. What is the final dilution?
• What would be the final volume of a diluted solutions that was made by diluting 250 mL a 4.5M solutions of H2SO4 to make a 3.5M solution? How much water would have to be added to reach the final volume?
• Question #811e2
• If 16.0 mL of water are added to 31.5 mL M #Ba(OH)_2(aq)#, what is the new solution molarity?
• Question #dc400
• #60# #mL# of a #1.5# #M# solution of #HCl# is diluted to a volume of #2.0# #L#. What is the concentration of the new solution?
• How do you find the density of a solution if you know the identity of the solute and solvent, the amount that you combine of each, and their individual densities?
• Dilution of a diprotic acid?
• How do we prepare #2*mol*L^-1# #HCl# from #16*mol*L^-1# #HCl#?
• Question #b886a
• Question #b889f
• Question #3e8e7
• What does it mean that a substance absorbs at #lambda_max#? How is absorbance related to concentration?
• A #"standard solution"# is #"aqueous"#, #"unsaturated"#, #"a mother solution"#?
• What volume of a solution that is #6.0*mol*L^-1# #HCl# is required to make #1.00*L# of a #0.10*mol*L^-1# solution?
• A certain amount of rubidium iodide was dissolved in #"4.6 L"#. A #"1-L"# aliquot was extracted an diluted to #"13.9 L"# to form a #"0.65 M"# solution in water. What mass of rubidium iodide was dissolved into the original solution?
• What is the #%"w/v"# of #"NaOH"# if #"4.0 g"# of it was in #"500 mL"# and #"10 mL"# of it was used to get #"100 mL"#?
• How much concentrated solution do you measure out and how much water do you need to add to make 500ml 0.1M HCl from 2M HCl?
• Question #e0ae8
• How do we make a #1*L# volume of a solution that is #0.5*mol*L^-1# with respect to #HCl# from a solution that is #10.6*mol*L^-1# with respect to #HCl(aq)#?
• Question #58587
• Question #7b280
• Question #30f4f
• Question #f5fb2
• Question #69542
• Question #33839
• What is the new concentration of a #10%# solution if we dilute a sample from #"25.0 mL"# to #"500 mL"# ?
• What the #"millimolarities"# with respect to sodium and chloride ions, of a #9.00*g# mass of sodium chloride dissolved in a volume of #1*L# of solution...?
• How many mmols in NaOH are used? In an experiment, 5mL of 6 M NaOH is used along with 300 ml distilled water. The solution of the NaOH was titrated into a vinegar solution and it was found that 7.92 mL of NaOH was used.
• Question #0cb6d
• Question #2b71d
• Question #b50ac
• Question #509f4
• What is the concentration in #"ppm"# when a #0.6068# mass of solute is dissolved in a #100*mL# of water?
• The concentration of a solution of ammonia, #"NH"_3# is #"1.5% m/v"#. What is the molar concentration of a solution produced by diluting #"25.0 mL"# of this solution with #"250 mL"# of water?
• Given #93.2%# #"w/w"# #"sulfuric acid"# that has #rho=1.835*g*mL^-1#, how should we dilute this to get a #3*N# solution of #0.50*L# volume...?
• Describe the difference between concentrated and dilute at the molecular level??
• Question #03a5a
• Question #cec3a
• Question #a673e
• Question #111d3
• What is the new concentration of a solute when a #20*mL# volume of a mother liquor at #2.0*mol*L^-1# concentration is diluted to a volume of #100*mL#?
• Question #11605
• What volume of #18*mol*L^-1# #H_2SO_4(aq)# is needed to make a #250*mL# volume of solution that is #0.50*mol*L^-1# with respect to #H_2SO_4#?
• Question #25bc8
• What volume of #84%# #HNO_3# #"w/w"#, #rho=1.54*g*mL^-1#, is required to make a #1.0*L# of a #1*mol*L^-1# solution of nitric acid?
• Question #6f783
• What is the dilution factor if a #0.1*mL# volume is diluted to #25.0*mL#?
• Given a #10*mL# volume of #10%# solution, what volume is necessary to make a #1%# solution?
• What is the volume of #2.0 # #mol# #dm^-3 # sodium chloride needed to prepare #250cm^3# of #0.2 ## mol# #dm^-3# sodium chloride solution ?
• How to prepare 0.2% of Hcl 36% in a water tank its volum is 5000 litre?
• How can we make 10 fold dilution when we only have 0.5 ml of stock solution?
• You are given a #"5-mL"# cell suspension with a cell count of #6.5 * 10^5# #"cell/mL"#. You are required to culture the cells at the density of #6.5 * 10^3# #"cell/mL"#. What dilution must you perform to obtain the required density?
• Question #51d88
• Question #cceac
• Question #f7dcc
• Question #98f95
• Question #11820
• Question #aa745
• Question #b8a58
• Which of the following corresponds to a final volume of a #12.89 * 10^(-3)# #"M"# solution prepared by the dilution of #"27.9 L"# of a #"433.0-mM"# solution?
• What weight of potassium permanganate is required to produce 300mL of solution such that 5mL of this solution diluted to 250mL gives a 0.01% w/v solution?
• Question #59b26
• Question #aa2dd
• Question #14c76
• What is the concentration of the solution produced when 150.0 mL of water is added to 200.0 mL of 0.250 M NaCl?
• What is the molarity of the solution produced when #"350.0 mL"# of water and #"75.0 mL"# of #"0.125 M"# #"NaNO"_3# are mixed an boiled down to #"325.0 mL"# ?
• Question #8d3d7
• #1.00 *10^2# #"mL"# of a #"12.4-M"# #"HCl"# solution is added to water to bring the total volume of the solution to #"0.820 L"#. What is the concentration of this new solution?
• How much (in #"L"#) of a #"1.2-M"# #"NaCl"# solution must be used to dilute to create #"1 L"# of a #"0.12-M"# #"NaCl"# solution?
• Suppose you wanted a 2:25 dilution of a stock solution, but you wanted 200 ml of it. How would you make this?