Answered: 25.0mL of 0.15 M boric acid (K, = 5.79…

25.0mL of 0.15 M boric acid (K, = 5.79 x 10) is titrated with 0.15 M NaOH. Find the pH at the following volumes of titrant: 1.0ml 12.5mL

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: A 50.0-mL sample of 0.15 M acetic acid, CH3COOH (Ka = 1.82 x 10-5 ), is titrated with 0.15 M NaOH…

A: Volume of acetic acid = 50 mLConcentration of acetic acid = 0.15 MConcentration of NaOH To…

Q: A 20.0-mL sample of a 0.125 M diprotic acid (H2A) solution is titrated with 0.1019 M KOH. The acid…

A: The neutralisation reaction taking place to reach first equivalence point is given by H2A + KOH…

Q: Calculate the pHpH at the equivalence point for titrating 0.240 MM solutions of each of the…

Q: Calculate the pH at the equivalence point for the following titration: 0.40 M HCl versus 0.40 M…

Q: The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid…

A: An acid is a substance that can increase the concentration of hydrogen ions () in the aqueous…

Q: 10.00 mL of 0.2357 M acetic acid {Ka = 1.80 xx 10^(-5)} is titrated with 0.1401 M NaOH. a) What is…

A: Given: The volume of acetic acid is 10 mL. The volume of NaOH is 8.240 mL. The molarity of acetic…

Q: For the titration of a weak acid with a strong base, such as acetic acid with sodium hydroxide, at…

A: Acetic acid is a weak acid and NaOH is a strong base.

Q: A 105.2 mL sample of 0.100 M methylamine ( CH3NH2; Kb = 3.7 x 10-4) is titrated with 0.270 M HNO3.…

A: Answer:- This question is answered by using the the simple concept of calculation of PH during the…

Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…

A: The objective of the question is to balance the given redox reaction under acidic conditions and…

Q: A 45.60-mL sample of a 0.476 M solution of acetic acid (HC2H3O2) which is a weak acid with an acid…

A: volume of acetic acid (H C₂ H 30₂) = 45.60 ml molarity of acetic acid = 0.476M Ка (H C₂ H…

Q: Consider the titration of 50.0 mL of 0.0500 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HI.…

A: a ) When 0.0 mL of acid is added , there is only base in solution so we would use its concentration…

Q: 25.0mL of 0.25M HBr is titrated with 0.10M NaOH. Which of the indicators below is the best choice to…

A: Interpretation - To tell about the indicator which is best choice to determine the endpoint when…

Q: Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (K, = %3D 6.3×10-5) by…

Q: A 103.8 mL sample of 0.105 M methylamine (CH3NH2;Kb = 3.7\times 10-4) is titrated with 0.260 M HNO3.…

Q: If 1. ml of 0.50 M formic acid (HCOOH) is titrated with the strong base of 0.50 M. KOH (Ka for…

A: The pH for the equivalence point : Balance chemical equation :…

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 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K = 0.000540) with 0.100 M HBrO…

A: HBrO4 is a strong monoprotic acid. (CH3)2NH is a weak monoacidic base (Kb = 0.000540 or 5.40x10-4)…

Q: A 25.0 mL sample of a 0.100 M solution of acetic acid is titrated with a 0.125 M solution of…

Q: Please answer with all equations worked out for the pH at 0, 25, 40, 50, 60mL of KOH Ionization…

A: Hi there! Since their are multiple subparts in the question, we will answer the first three subparts…

Q: A 15.00 mL sample of 0.355 M H3PO4 (Ka,1 7.52 ´ 10–3 , Ka,2 6.23 ´ 10–8 , Ka,3 2.1 ´ 10–13) is…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

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: Calculate the pH in the titration of 50.00 mL of 0.060 M acetic acid (CH3COOH) with a 0.120M sodium…

A: (A)pH when 0mL of NaOH solution is added:

Q: A 65.0 mL solution of 0.158 M potassium alaninate ( H, NC, H, CO, K) is titrated with 0.158 M HCI.…

Q: If someone takes a breath and the lungs expand from 4.5 L to 5.8 L in volume, and the initial…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A: (a) The formula to calculate the moles from molarity is as follows: Moles=MolarityVolume…

Q: solution is made by mixing 0.250 L of 0.020 mol L-1 acetic acid and 1.10 g of potassium acetate (M =…

A: Here a solution contains 0.25 L of 0.02M acetic acid and 1.10 g of CH3COOK. Ka CH3COOH =1.8×10-5 .…

Q: 25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50 M NaOH. Calculate the…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Titus titrates 60 mL of 0.700 M lactic acid (HC,H,O,, Ka = 1.5 × 10 NaOH. Calculate the pH of the…

Q: Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb= 5.2 x…

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: Which indicator is the best to use for the following titration? Strong Acid with Weak Base…

A: Titration is a volumetric analysis which is used to measure the volume of an unknown compound. The…

Q: I Draw structures corresponding to the given names. p-iodo aniline 2-ethyl-4-methyl acetophenone

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: o A 55.0 mL solution of 0.150 M potassium alaninate ( H₂NC₂H₂CO₂K) is titrated with 0.150 M HCl. The…

Q: A 50.0 ml aliquot of a 0.0010OM solution of acetic acid (K = 1.8 x 10-5) is titrated with 0.00993M…

Q: Calculate the pH at each point in the titration of 20.0 mL of 0.125 M weak acid, HA, with a Ka value…

Q: Consider the titration of 40 mL of 0.2 M NH3 with 0.5 M HCI. Calculate the pH after addition of the…

A: In this question it is ask that what is the pH of resultant solution when addition of HCl in NH3 as…

Q: You have 10 mL of a buffer that is 0.1 M acetic acid and 0.1 M sodium acetate. How many mLs of 0.025…

A: The number of moles of acetic acid and sodium acetate in the 10.0 mL of buffer is;…

Q: Use an Excel spreadsheet to generate a titration curve for 50.00 ml. of 0.0200 M acetic acid (K, =…

A: The balanced chemical equation for the reaction between acetic acid and ammonia is:…

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

12.
25.0mL of 0.15 M boric acid (K, = 5.79 x 10) is titrated with 0.15 M NaOH. Find the pH at the following
volumes of titrant:
1.0mL
12.5ml
26.0mL
45.0mL

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 with 2 images

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

Consider the titration of 40.0 mL of 0.0600 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HI. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 6.0 mLpH = (c) 12.0 mL
Consider the titration of 40.0 mL of 0.0600 M C6H5NH2 (a weak base; Kb = 4.30e-10) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 6.0 mLpH = (c) 12.0 mLpH = (d) 18.0 mLpH = (e) 24.0 mLpH = (f) 45.6 mLpH =
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H,NNH2 with 0.100 M HNO, after 80.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 x 10-6.
10.00 mL of 0.2099 M iodic acid {Ka = 1.70 xx 10^(-1)} is titrated with 0.1057 M NaOH. a) What is the pH after 14.61 mL of NaOH are added to the solution?
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:
The titration of CH3COOH (Ka = 1.76x10-4; pKa = 3.754; Kb = 5.68x10-11) with NaOH is an example of a weak acid/strong base titration. A 40 mL aliquot of a 0.060 M solution of HCOOH is titrated by 0.060 M KOH. What is the pH of the solution at each of the following points: a) initially b) after 1 mL of base has been added c) after 20 mL of base has been added d) at the equivalence point e) after 45 mL of bases has been added
Be sure to answer all parts. Use the figure below to find an indicator for these titrations: (a) 0.10 M CH3NH₂(Kb = 4.4 x 10-4) with 0.10 M HCI (select) (b) 0.50 M HI with 0.10 M KOH (select) Crystal violet Thymol blue 2,4-Dinitrophenol Bromophenol blue Bromocresol green Methyl red Alizarin 0 Bromothymol blue Phenol red Phenolphthalein Alizarin yellow R 11 12 13 14
(a) A 25.0 mL sample of 0.175 M methylamine CH3NH2 (Kb = 1.3 x 10-5) is titrated with 0.150 M HBr. Find the initial pH at the ½ equivalence point after 5.0 mL of acid is added the pH at the equivalence point the pH after 5.0 mL acid is added after the equivalence point
Determine the pH during the titration of 60.4 mL of 0.442 M formic acid (Ka = 1.8×10-4) by 0.442 M KOH at the following points. At the equivalence point (e) After the addition of 90.6 mL of KOH