THIS IS 1 OF 2I'm uploading the other 2 images that go with these next, because the limit shows 2 images DATAMass of NaCl needed for 50.0 mL of 0.200 M NaCl solution(Show calculation below.)pH afteraddition ofChange in pHfrom initialInitial pHpH afteraddition ofChange inpH frominitialstrong acidstrong base7.052.45WaterI1.8917.092.474.62/456Lo.75 0.700.200 MNaClacetate4.70bufferphosphatebufferQUESTIONSDo chloride or sodium ions have a big effect on pH? What is the evidence that supports youranswer? (Hint: Compare the initial pH's of water and 0.200 M NaCl.)1.2.Is the 0.200 M NaCl solution buffered or not? What is the evidence that supports your answer? Saline is another name for a solution containing sodium chloride. Severely dehydrated patientsmay be given a buffercd saline solution intravenously to restore their fluid balance. Do you thinkthat a buffered saline solution would contain only sodium chloride in the solution? Justify youranswer using your experimental evidence.3.4.Use the dilution equation to calculate the number of milliliters of 3.00 M NaCl needed to make600.0 mL of a saline solution with a final sodium chloride concentration of 0.154 M. Show yourwork.5.Calculate the molarity of a solution made by dissolving 85.0 grams of Na;SO4 in enough water tomake 250.0 mL of solution. Show your work.

Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Mass of NaCl needed for 50.0 mL of 0.200 M NaCl solution. (Show calculation below.) Change in pH from initial pH after addition of Change in pH from initial Initial pH pH after addition of strong acid strong base 7.05 .45 7.092.47 4.62456 phosphate lo.75 .70 Water 11.89 0.200 M NaCl acetate 4.70 buffer buffer L6,70 QUESTIONS 1. Do chloride or sodium ions have a big effect on pH? What is the evidence that supports your answer? (Hint: Compare the initial pH's of water and 0.200 M NaCl.) 2. Is the 0.200 M NaCl solution buffered or not? What is the evidence that supports your answer?

Mass of NaCl needed for 50.0 mL of 0.200 M NaCl solution. (Show calculation below.) Change in pH from initial pH after addition of Change in pH from initial Initial pH pH after addition of strong acid strong base 7.05 .45 7.092.47 4.62456 phosphate lo.75 .70 Water 11.89 0.200 M NaCl acetate 4.70 buffer buffer L6,70 QUESTIONS 1. Do chloride or sodium ions have a big effect on pH? What is the evidence that supports your answer? (Hint: Compare the initial pH's of water and 0.200 M NaCl.) 2. Is the 0.200 M NaCl solution buffered or not? What is the evidence that supports your answer?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

See similar textbooks

Similar questions

. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Give only typing answer with explanation and conclusion to all parts Calculate the concentrations of all species in a 0.490 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are ?a1=1.4×10−2 and ?a2=6.3×10−8. [Na+]= [HSO−3]= [OH−]= [SO2-3]= [H2SO3]= [H+]=
For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surely
Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the total vol. of buffer
A 20-mL vial of concentrated ammonium chloride solution containing 5 mEq/mLis diluted to 1 liter with sterile distilled water. Calculate (a) the total milliequivalent value of the ammonium ion in the dilution and (b) the percentage strengthof the dilution.
At 25oC, a 50mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of the solution is 1.05g/cm3 . If this solution is diluted further to form 500mL, what will be the: A) [OH- ] B) pH C) % dissociation of the resulting acetic acid solution?
Need solution urgently 125mL of an alkaline water sample containing 128 ppm carbonate and 40ppm hydroxide in terms of CaCO_(3) equivalent its titrated against 0.20NHCl using methyl orange as the indicator.What will be the titre value (in ml unit)?
equal volumes of 0.15M sulfurous acid and 0.3M potassium hydroxide are moxed. write net ionic and identify spe ies with highest concentration at equlibrium. Please explain justification
Consider the Heat of Solution Practical that was conducted. Temperature (oC) Amount of NaOH ( 0.015M) used to reach end point of titration (ml) 40 42 35 35 30 26 25 23 20 16 Use the data provided above in order to determine the heat of solution. Include any necessary graphs.
A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.
An aqueuous solution of K3PO4 would be...a) either acidic or basic depending on the amount of salt dissolved. b)basicc) acidicd) neutrale) either acidic or basic depending on the actual values of Ka and Kb which must be known.
Determination of Ksp value given concentration of Ca2+ is 7.72705 ppm, and pH =9.24, and chemical equations (some sort of derivation using these equations and above values is needed to calculate the Ksp value)