182183134185FABEDC1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE tableand Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical186187188400190191192193195ReactionInitial conc. / M:Change in conc. at equilibrium/M:Equilibrium conc. / M:pHHA(aq) + H₂O(l)0.19792.946990323-2.2E-042. Use your data and the Henderson-HasselbalchpH=pka + log[A]/[HA] and1.98E-01Ka =2.5E-07pKa pH-log[A]/[HA]=pkaH3O*(aq)05.9E+002.2E-042.2E-04+equation to perform the calculation and find Ka at any pH during titration.Ka = 10 KaA (aq)ᏅKa2.2E-042.2E-041.3E-06Hints:Use Ex pH 2.946990323Comparison of Results:pka1 At 5.00 mL of NaOH before the equivalence point2 At the equivalence point3 At 5.00 ml after the equivalence point5.9E+00Ka1.3E-06LC POST-LAB QUESTIONSThese are OPTIONAL questions that can be used either as EC or as a substitute for the Module QuizUsing experimentally determined values of Ka and molarity of your acid solution and the concentration of the standardized NaOH solution, calculate the pHof the following points of your titration curve (check examples provided in the Lab Manual Manual):

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

E D C B 1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical A (aq) H.O*(aq) oll +

E D C B 1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical A (aq) H.O*(aq) oll +

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: What is the pH of a 75.0 ml of a 0.1 M pyridine (C5H5N) solution (Kb= 1.7 x 109) when 100.0 mL of a…

Q: Determine the pH at the point in the titrátion of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

A: Base dissociation constant , Kb represents basicity in a solution. For a dissociation of base (B) in…

Q: Calculate the hydronium ion concentration and the pH when 35.0 mL of 0.45MN*H_{3} is mixed with 35.0…

Q: Calculate an unknown concentration of a NaOH solution if 0.224 g of oxalic acid, H2C2O4*2H2O,…

A: Molar mass of H2C2O4.2H2O = 126 g/mol Calculation of no. of mol of Oxalic Acid: According to the…

Q: In part one if you allow your titration to go beyond a faint pink endpoint and it ends up dark pink,…

A: Given: Trial-1 Trial-2 Molarity of HCl 31.34 31.44

Q: An analytical chemist weighs out 0.413 g of an unknown diprotic acid into a 250 mL volumetric flask…

Q: A chemist titrates 180.0 mL of a 0.4899M potassium hydroxide (KOH) solution with 0.5114M HCl…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: Determine the acid dissociation constant, Ka, for a 0.10 Ma weak acid solution that has a pH of…

A: Given : Concentration of weak acid HA = 0.10 M And pH of the solution = 2.87 The ionisation…

Q: a. Using the Bohr model of the atom, calculate the wavelength, frequency, wavenumber, and energy per…

Q: A monoprotic acid HX has Ka = 1.3 × 10¬³. Calculate the equilibrium concentrations of HX and H3O*…

Q: Answer the questions based on the titration of 250.0 mL of 0.400 M A- with 0.637M HCl at 25 oC. (Kb…

A: Q.1: pH prior to the addition of any acid: Since A-(aq) is a weak monoprotic base, it will form…

Q: An analytical chemist weighs out 0.133 g of an unknown diprotic acid into a 250 mL volumetric flask…

Q: Calculate the pH of a solution containing a salt B Cl derived from a strong acid (HCl) and a weak…

A: The concentration of hydrogen ion in the salt solution is calculated as shown below where C is the…

Q: Write the acid dissociation chemical equation, including states of matter, associated with the pH 7…

A: Phosphoric acid is a tribasic acid and it dissociates in three steps. The dissociation of phosphoric…

Q: 50.0 mL of 0.050 M KOH(aq) is titrated with 0.10 M HCI (aq). Calculate the pH at each volume of acid…

Q: Determine the Ka value [H +]eq Solution 1 3.98 X 10-3 M Solution 2 6.03 X 10-4 M Solution 3…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: A CHM 122 student performs a titration with 28.5 mL of 0.25 M weak acid solution witha 0.25 M LIOH…

A: GIVEN: The Volume of weak acid = 28.5 mL Concentration of weak acid= 0.25 M Concentration of Base=…

Q: Using only the Henderson-Hasselbalch equation, what is the pH of a solution that is 0.22M phenol,…

A: Given: Molarity of phenol = 0.22 M Molarity of sodium phenoxide = 0.29 M Ka of phenol = 1.3×10-8

Q: Chadwick the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

A: Chadwick the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

Q: 2 An analytical chemist is titrating 72.5 mL of a 0.6200M solution of propionic acid (HC,H,CO,) with…

A: In first step, we calculate moles of acid and base by multiplying their molarity with volumes. nbase…

Q: d. Oxalic acid (H2C2O4) is the compound that gives rhubarb its tart flavor, and it is also a toxin…

A: The question is based on the concept of molarity.Molarity is a method of expressing concentration of…

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: The student Louise continued the analysis of acetic acid using half - neutralization technique. She…

A: pH of any solution is given by pH = -log[H3O+ ] where [H3O+ ] = molar concentration of H3O+

Q: What is the final ph of a solution obtained by mixing 100ml of 0.15 M NH3 with 75 ml of 0.10 M HCl?…

Q: which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was…

A: The question is based on the concept of solutions. we have to quantitatively estimate the citric…

Q: Buffers 1. Determine the pH of a solution that contains 0.376 M hydrogen phosphate (HPO ) and 0.468…

Q: Window cleaner Seltzer water Antacid tablets Aspirin tablets green Blue light blue red pink 11 7 8 2…

A: pH of a solution is the negative logarithm of the value of the molar concentration of H3O+ ions in…

Q: Complete the balanced neutralization equation for the reaction below: H2SO:(aq) + Mg(OH):(aq) –

A: To complete the balanced neutralization reaction H2SO4 (aq) + Mg (OH)2 (aq) ----------->

Q: Benzoic acid, HC7H5O2, has a Ka value of 6.4 x 10-5. 1. Find the pH of a 1.50 M solution of benzoic…

A: Hi! Thank you for the question, As per the honor code, we are allowed to answer one question at a…

Q: Haley conducted a titration experiment of a waek acid and stong base. For the experiment she used…

A: Titration is an analytical technique in which an unknown concentration of a solution is determined…

Q: Calculate the unknown concentration of an NaOH solution if 0.224 g of oxalic acid, H2C2O4*2H2O,…

A: NOTE : The reaction given is incorrectly balanced. I have correct the balancing in the below…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

182
183
134
185
F
A
B
E
D
C
1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table
and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical
186
187
188
400
190
191
192
193
195
Reaction
Initial conc. / M:
Change in conc. at equilibrium
/M:
Equilibrium conc. / M:
pH
HA(aq) + H₂O(l)
0.1979
2.946990323
-2.2E-04
2. Use your data and the Henderson-Hasselbalch
pH=pka + log[A]/[HA] and
1.98E-01
Ka =
2.5E-07
pKa pH-log[A]/[HA]
=
pka
H3O*(aq)
0
5.9E+00
2.2E-04
2.2E-04
+
equation to perform the calculation and find Ka at any pH during titration.
Ka = 10 Ka
A (aq)
Ꮕ
Ka
2.2E-04
2.2E-04
1.3E-06
Hints:
Use Ex

pH 2.946990323
Comparison of Results:
pka
1 At 5.00 mL of NaOH before the equivalence point
2 At the equivalence point
3 At 5.00 ml after the equivalence point
5.9E+00
Ka
1.3E-06
LC POST-LAB QUESTIONS
These are OPTIONAL questions that can be used either as EC or as a substitute for the Module Quiz
Using experimentally determined values of Ka and molarity of your acid solution and the concentration of the standardized NaOH solution, calculate the pH
of the following points of your titration curve (check examples provided in the Lab Manual Manual):

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI
Please help in solving e-f of question. Thanks
||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…
Calculate the pH of a solution containing 23 mL of 1.54 M of a weak weak base B OH, like NH4OH, or simply written as NH3, titrated with 17 ml of 1.01 M a strong acid AH, for instance HCl. The base dissociation constant, Kb , is 1.00e-5. pH ← please insert your value
Determine the molarity of a 7.00 ml HCl solution if it takes 48.35 mL of a0.1315M NaOH solution to neutralize in a titration. HCl+NaOH-->NaCl +H2O
A 0.453 g sample of a diprotic acid is dissolved in water and titrated with 0.200 M NaOH. What is the molar mass of the acid if 34.8 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol 10 11 16 17 18 19 20 21 22 23 24 5