28/03/2021, 4:34 PMam/forms/d/e/1FAlpQLSd7Qir0XcW1yfDw7IHKj570x6qm-viAIM52kD5hE8L98ycvaQIn titrating 10 ml of 0.1 N HA (pKa-D4),the pH after the addition of 12 ml 0.1NNaOH is3.6911.213.813.2112.314.5010.313.311.3O 2.69Submit

Given Normality of HA = 0.1 N Volume of HA = 10 mL Mole of HA = Normality of HA * Volume of HA Mole…

Answered: In titrating 10 ml of 0.1 N HA…

In titrating 10 ml of 0.1 N HA (pKa-4),the pH after the addition of 12 ml 0.1N NaOH is O 3.69 О 11.2 13.8 13.21 12.31 O 4.50 О 10.3 O 13.3 O 11.3 O 2.69

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: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl. Carbonic acid (H2CO3) has a…

A: The number of milliequivalents of sodium carbonate Na2CO3 = 40.00 x 0.1250 = 5 mmol The number of…

Q: A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer…

Q: Which of the following mixtures of acids exhibit(s) two end points when titrated with 0.10 M NAOH? O…

A: Option b is correct.

Q: OO O O O A 25.0-ml sample of 0.175 M C2H5NH2 is titrated with 0.150 M HCI. What is the pH at the…

A: Given, Molarity of C2H5NH2 = 0.175 M Volume of C2H5NH2 in mL = 25.0 mL Molarity of HCl = 0.150 M…

Q: Calculate the pH during the titration of 20.0 mL of 0.10 M Ammonia (Ka = 1.8 × 10-5) after the…

A: This is weak base strong acid titration Where pH can be calculated using Henderson-Hasselbalch…

Q: Calculate the pH at the equivalence point for the following titrations. 4A. Benzoic 50. mL of 0.12 M…

A: Given,4A) Molarity of benzoic acid = 0.12 Mvolume of benzoic acid = 50. mLMolarity of potassium…

Q: Please answer part A. Thank you!

A: The indicators which are used to determine the end point are known as acid- base indicators. The…

Q: A 75.0 mL sample of 0.05 M HCN (pKa = 9.21) is titrated with 0.5 M NAOH. What is [H3O*] in the…

Q: A buffer solution containing only 0.050 mol of CH3NH2 and 0.060 mol of CH3NH3CI has a total volume…

A: Given: Moles of CH3NH2 = 0.050 mol. Moles of CH3NH3Cl = 0.060 mol. And the moles of NaOH added =…

Q: Calculate the pH at the equivalence point in titrating 0.028 M solutions of each of the following…

A: a)

Q: What is the effective pH range of a buffer (relative to the pKa of the weak acid component)? pKa +3…

A: The effective pH of a buffer or weak acid can be determined by using Henderson Hasselbalch equation.…

Q: Sketch the titration curve for the titration of 85 mL of 0.40 M A− (Kb = 3.9 ✕ 10−7) with a 0.40 M…

Q: A 30.0 mL sample of 0.200 M hypochlorous acid (HClO; Ka = 30.0 x 10-8) is titrated with 0.100 M KOH.…

A: To calculate the pH of the solution when the below volume of 0.100 M KOH is added to a 30.0 mL…

Q: In the titration of 50.0 mL 0.20 M acetic acid with 0.40 M NaOH, what is the pH of the solution…

Q: A 50.00-mL sample of 0.0750 M HCN was titrated with 0.3995 M NaOH. What is the pH at the equivalence…

A: The objective of this question is to calculate the pH at the equivalence point of a titration…

Q: Calculate the pH for a buffer made with 230.0 mL of 0.189 M furoic acid (HC5H3O3) and 20.0 mL of…

Q: 16. What is the solubility of Ca(OH)2 in 0.0860 M Ba(OH)2? The Ksp for Ca(OH)2 is known to be 4.68 x…

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

Q: A 20.0 mL sample of 0.150 M ethylamine is titrated with 0.0981 M HCI. What is the pH after the…

A: Given mmoles of base = 0.15 M x 20 mL = 3 mmoles of acid = 0.0981 M x 5 mL = 0.4905…

Q: What is the pH of a buffer made by dissolving .762 g of HCHO2 and .212 of KCHO2in 1.0 L of solution?…

A: Here the buffer solution is made with weak acid, HCHO2, and its conjugate base KCHO2 in a 1L…

Q: Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP…

Q: Consider a monoprotic acid titrated with NaOH. 14.0 12.0 10.0 8.0 pH 6.0 4.0 2.0 0.0 0.0 10.0 20.0…

A: The equivalence point is at pH = 7 The volume of titrant added to reach equivalence point is = 35…

Q: Consider the titration of 500 mL of 100 mM boric acid. The pka of boric acid is 9.23. What will the…

A: Boric acid formula is which react with sodium hydroxide to form .Reaction is

Q: 24.1 ml sample of 0.644 m formic acid (hcho2) is titrated with 0.644 m naoh. calculate the ph after…

A: Given: Concentration of HCOOH = 0.644 M Volume of HCOOH sample = 24.1 mL = 0.0241 L…

Q: What is the pH at the 2nd half-equivalence point for the titration of 25.0 mL of 0.247 M diprotic…

A: Equivalence point is the point in the titration is where the concentration of the acid and the base…

Q: A buffer solution containing only 0.050 mol of CH3NH2 and 0.060 mol of CH3NH3CI has a total volume…

A: When sodium hydroxide is added then hydroxide ion is react with salt and produced base of basic…

Q: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl. Carbonic acid (H2CO3) has a…

Q: Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3…

Q: In the titration of a 30.0-mL sample of 0.115 M H2C6H6O6 with 0.130 M LIOH, where Ka, H2C6H6O6 =…

A: Half equivalence point means the concentration of acid and salt are equal ([Acid] = [salt]).…

Q: A buffer was prepared by adding 220.0 mL of 0.50 M NH3 solution to 280.0 mL of 0.20 M NH4Cl…

A: The pH of the solution (a) is; The concentration of NH3 in 500.0 mL of solution is;NH3=0.50 M×220.0…

Q: Vhat is the pH of a buffer that consists of 0.20 M NaH,PO4 and 0.40 M Na,HPO4? Ka1 = 7.5x 103 Ka2 =…

A: Given: Concentration of NaH2PO4 = 0.20 M Concentration of Na2HPO4 = 0.40 M

Q: In the titration of 50.0 ml of 0.1 M formic acid (ka- 1.8x 10) with 0.1M NAOH, what will be the pH…

Q: (a) A 5.0 mL sample of 0.175 M methylamine CH3NH2 (Kb = 1.3 x 10-5) is titrated with 0.150 M HBr.…

A: The objective of this question is to calculate the pH at various points during the titration of a…

Q: 1) What is the predominant form of the acid when the solution has pH=3.6. H2A HA- A^2- none of…

A: Given that The acid's pKa values of diprotic Acid are 2.81 and 5.74.

Q: Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3…

Q: How many grams of solid potassium hypochlorite should be added to 1.50 L of a 0.0598 M hypochlorous…

Q: 17- Consider the following titration curve that corresponds to the titration of a weak acid with a…

Q: A flask contains 50 mL of a buffer that is 0.10M in acetic acid and 0.20 M in acetate ion. What will…

A: We have to calculate the pH value.

Q: What is the pka of the weak acid that gives the following pH curve when titrated with NaOH? 14.00…

A: The value of pH for titration of weak acid with strong base is calculated by Henderson-Hasselbalch…

Q: Titration volume to pH 5.5 using 5.3mM HCl (0.0053 M): Sample Titre (mL) 1a 25.20 1b 25.40 1c 25.35…

A: The objective of this question is to given chemical system, we encounter three key species: the…

Q: Chemistry Refer to the acid-base titration curve shown below. What is the pKb of the base present at…

Q: in the titration of 50.0 mL 0.0200 M weak acid HA using 0.0150 M NaOH, what is the solution pH at…

A: Number of moles = Molarity x volume (L) Molarity of HA = 0.0200 M Volume of HA = 50.0 mL = 0.050 L…

Q: Calculate the ratio of KOAc to HOAc required to create a buffer with a pH of 3.92. For HOAc pka…

Q: For the titration of a weak acid with a strong base, the pH at the midpoint was 5.06. What are the…

A: I

Q: (HC6H5CO2) solution. Benzoic acid is a weak acid with K= 6.3x 10-5 . What mass of NaC6H5CO2 should…

A: Given, Molar mass of Acid = 144 g/mol Molarity of acid = 0.30 M Volume of Acid = 500 mL = 0.50 L…

Q: Suppose you have a buffer, comprised of 0.350 mol of weak base and 0.250 mol of weak acid. If the…

A: Given : A buffer solution with a weak acid and its conjugate base i.e weak base. Moles of conjugate…

Q: What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.29? See the Solubility…

Q: What is a pH at the equivalence point when exactly 25.00 mL of 0.1000 M (CH3)2NH is titrated with…

A: In this question we want to determine the pH of the Solution at Equivalence point. You can see…

Q: Calculate the pH in the titration of 100.0 mL of 0.20 M HCIO (Ka = 4.0 × 10^-8) with 0.20 M KOH…

A: Answer: This question is based on salt hydrolysis where salt of weak acid and strong base gets…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

28/03/2021, 4:34 PM
am/forms/d/e/1FAlpQLSd7Qir0XcW1yfDw7IHKj570x6qm-viAIM52kD5hE8L98ycvaQ
In titrating 10 ml of 0.1 N HA (pKa-D4),the pH after the addition of 12 ml 0.1N
NaOH is
3.69
11.2
13.8
13.21
12.31
4.50
10.3
13.3
11.3
O 2.69
Submit

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H 2PO 4 - and 0.100 M HPO 4 2- and the Ka2 = 6.2 × 10 -8? A 5.21 B 7.69 C 6.73 D 5.61
16.0mL of a 0.750M solution of H>COz are titrated with a 1.0OOM solution of KOH. At what volume of base will the equivalence point be reached? 42.7 mL 12.0 mL O24.0 mL 20.0 mL 21.3 mL
26 mL of 0.11 M acetic acid solution is titrated with 0.10 M NaOH. What is the pH after 12 mL of NaOH have been added? (Ka for acetic acid = 1.8 x 10-5)
What is the pH of a buffer that is 120 M in formic acid, HCHO2 and 0.080 M in potassium formate KCHO2? Ka(HCHO2) = 1.8 x 10-4 33 57 74 91
22
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N, with 0.1000 M HCl solution after the following additions of titrant. 10.00 mL: 21.00 mL: 28.00 mL:
Consider the titration of 55.0 mL of 0.120M nitrous acid (HNO2, K, = 4.5 x 10-4) with 0.100 M NaOH. What is the pH after adding 35.0 mL of base? O 6.03 O 3.51 O 3.40 O 7.97 O 3.29
A buffer solution is 0.500 M in KF and 0.500 M in HF (KA = 3.5 × 10–4). What is the solution’s pH after 0.200 moles of solid CsOH is added to 3.00 L of buffer solution? Assume that no volume change results from the addition of the CsOH. 3.09 4.46 3.82 3.22 3.57
10.0 mL of 0.02 M carbonic acid (H2CO3) is titrated with 0.01 M NaOH. What is the pH after 20.0 mL of NaOH is added? For carbonic acid, Ka1= 4.2 x 10-7, Ka2=4.3 x 10-11
Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10–5. What is the pH at the equivalence point?
which of the following acids (listed with pKa values) and their conjugate base would form a buffer with a pH of 8.10? (see image)
What is the pH of a buffer that is 120 M in formic acid, HCHO2 and 0.080 M in potassium formate KCHO2? Ka(HCHO2) = 1.8 x 10-4 3.3 5.7 7.4 9.1