What's in your Bucket (write the molecule and what type--WB, WA, SA, SB, buffer, or water) before and after adding 2.5 mL of 1.0M NaOH? Estimate the pH (<< 7 = SA, < 7 = WA, = 7 neutral, >7 WB, >> 7 SB). Write all reactions and/or chemical equilibrium shifts that occur and show all stoichiometry. 1) Soml of a1 mHCl and o.2m(CH,)N Before After

What's in your Bucket (write the molecule and what type--WB, WA, SA, SB, buffer, or water) before and after adding 2.5 mL of 1.0M NaOH? Estimate the pH (<< 7 = SA, < 7 = WA, = 7 neutral, >7 WB, >> 7 SB). Write all reactions and/or chemical equilibrium shifts that occur and show all stoichiometry. 1) Soml of a1 mHCl and o.2m(CH,)N Before After

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 16.52QE

See similar textbooks

Similar questions

Which of these procedures would not make a pH =4.75buffer?(a) Mix 50.0 mL of 0.10 M acetic acid and 50.0 mL of 0.10 M sodium acetate.(b) Mix 50.0 mL of 0.20 M acetic acid and 50.0 mL of 0.10 M NaOH.(c) Start with 50.0 mL of 0.20 M acetic acid and add a solution of strong base until the pH equals 4.75.(d) Start with 50.0 mL of 0.20 M HCl and add a solution of strong base until the pH equals 4.75.(e) Start with 100.0 mL of 0.20 M sodium acetate and add 50.0 mL of 0.20 M HCl.
Prior to making buffer X, you need to prepare the requisite stock solutions. Describe how you would make 100 mL of each stock solution: 1M NaCl, starting with crystalline NaCl (molecular weight 58.44) 1M Tris, starting with crystalline Tris (molecular weight 121.1 1M MgCl2, starting with crystalline MgCl2 (molecular weight 95.2)
How many mls of 1 M NaOH titront are needed to react with 5 mls of 0.1 KHT? (Use the ml*M/ coefficient= ml*m/coefficient formula to solve this problem)
How many ml of 0.2 M HCl needs to be added to 100.0 ml of 0.2 M Sodium acetate (kb for acetate is 5.6x10-10 to achieve a pH of 4.5?
How will you prepare a pH 4.50 acetic acid-acetate buffer such that when1.00 mL of 10 M NaOH is added to 100.00 mL of this buffer, the resulting pHwill be raised by exactly 1 pH unit? Show calculations for the concentrations(in 3 decimal places) of the components that must be present in the bufferas well as the volumes of 1 M acetic acid and 1 M sodium acetate that needto be mixed and diluted to 100.00 mL to prepare the buffer. (There is nospecific final buffer concentration required here. You can verify your answersby using the Virtual Lab).
I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)
How to answer for Ka/ Kb and calculated pH of a solution? I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Ex. Solution 1: 30.0 mL 0.10 M CH3COOHSolution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COOSolution 3: 30.0 mL 0.10 M NH3Solution 4: 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl Sol 1,2 used methyl orange as indicatorSol 3,4 used phenolphthalein as indicator Solution w/ measured pH Ka/Kb Calculated pH 1 a 1.0 M HCl (2.01pH) b 1.0 M NaOH (3.98pH) c Control (2.91pH) 2 a 1.0 M HCl (4.73) b 1.0 M NaOH (4.82) c Control (4.76) 3. a 1.0 M HCl (10.09) b 1.0 M NaOH (11.98) c Control (11.11) 4. a 1.0 M HCl (9.13) b 1.0 M NaOH (9.38) c Control (9.30)
Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.
By reference to the reacting ratio of HCL and NaOH, deduce the number of moles of NaOH required to reach Equivalence. Btw I did the first part of the question so this is a follow up.
Does my math add up? Calculate the moles of NaOH delivered at the equivalence point as determined by the second derivative plot for your careful trial, then enter the values in Table 2. 24.178(mL) x 1 / 1000 (mL) x 0.1002(M) = 0.0024709916 mol = 2.47 x 10 ^ -3 mol Calculate the number of moles of HCl as experimentally determined by the titration into Table 2. 2.47 x 10 ^ -3 mol Calculate the concentration of the original HCl solution for then enter the values in Table 2. M = n / VL = 2.47 x 10 ^-3 / 10 x 10 ^-3 = 0.247 molar Table 2. Second Derivative Processed Data Trial 2 moles of NaOH at equivalence point 2.47 x 10 ^ -3 moles of HCl 2.47 x 10 ^ -3 concentration of original HCl solution (M) 0.247
Compute for the titratable acidity of vinegar sample if 6 ml of 1.0 N NaOH was used to titrate 25 ml of sample. Can this sample be used commercially if the standard is 4% titratable acidity?
Considering the equilibrium below, which of the following is/are TRUE? CH3OH + HNO2 = CH3OH2+ + NO2- CH3OH is a base NO2 is a conjugate acid IAM. I only SXY. II only AND. I and II IKI. Neither I nor II Which of the following statements is/are ALWAYS TRUE? A higher Ksp value equates to a higher solubility regardless of the salt type When Qsp = Ksp, the system is at equilibrium CHM. I only EQU. II only LIB. I and II RIA. Neither I nor II