Answered: 8. A 100. mL sample of 0.10 MHCI is…

8. A 100. mL sample of 0.10 MHCI is mixed with 50. mL of 0.12 M NH.. What is the resulting pH? (K, for NH3 = 1.8 × 10-- 3.07 10.93 1.57 12.43 1.40

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: Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K = 3.5×108) by 0.467…

A: Given that : The volume of hypochlorous acid = 26.8 mL The molarity of hypochlorous acid = 0.447 M…

Q: A solution of is known to contain 0.100 M pyridine and 0.300 M pyridinum hydrochloride. The Kb for…

A: The determination of H+ ions which are available in any specific solution is carried out with the…

Q: Al of the folowing lonic compounds are only slightly soluble in pure water Which of those wil show…

A: A question based on solutions that is to be accomplished.

Q: A 25.5 mL sample of 0.361 M trimethylamine, (CH3)3N, is titrated with 0.300 M hydroiodic acid. After…

A: By using Henderson hasselbalch equation we can find the pH of solution.

Q: What is the pH if 0.188 L of 0.206 M KOH is added to the solution be?

Q: What is the weight NaCH3COO of that must be added to 750.0 mL of 0.180 M acetic acid to form a pH =…

A: Recall Henderson-Hasselbalch equation for acidic buffer solution pH=pKa +…

Q: Since phosphoric acid is polyprotic, it can create several buffer regions. One buffer forms between…

Q: Determine the pH during the titration of 58.3 mL of 0.310 M acetic acid (K, = 1.8×10) by 0.310 M…

Q: A solution of HA (0.197M; 81.7mL; Kp =5.5E-7) is titrated with 0.4334M KOH. Determine the pH at the…

A: pH of solution at different points can be calculated using Henderson hasselbalch equation.

Q: to the solution containing 8 grams of Ca (OH) 2 in 50 ml of it add 500 ml of solution 0.1 mol HCl…

A: Given, Mass of Ca(OH)2 = 8 grams Volume of Ca(OH)2 = 50 ml = 0.05 L Volume of HCl = 500 ml = 0.5 L…

Q: Determine the pH during the titration of 66.5 mL of 0.376 M acetic acid (K, 1.8x105) by 0.376 M KOH…

Q: Question 17 of 25 Submit Which of the following combinations can be used to make a buffer? (Assume…

A: A buffer solution resist the change in pH when small amounts of acid or base is added .it is of two…

Q: Titrate in 26 ml of 2.2 M NaOH into 1200 ml of .5M HCO2H, what will the pH?

Q: A solution is prepared that is initially 0.36M in trimethylamine ((CH3),N), a weak base, and 0.19M…

Q: 73. A student dissolves 0.0100 mole of an unknown weak base in 100.0 mL water and titrates the…

A: First determine the mole of HNO3 present in 40mL of solution. The excess base present after…

Q: A handbook states that to prepare 100.0 mL of a particular buffer solution, mix 63.0 mL of 0.200 M…

A: Given, Volume of the buffer = 100.0 mL Volume of the HC2H3O2 = 63.0 mL Molarity of HC2H3O2 =…

Q: You have 75.00 mL of a 0.25 M NaOH solution that you are going to titrate with 0.5M Hal. What is…

A: (a)Initial pH:

Q: Caleulate the pH of the solutions. Buffer 1: 25.0 mL of 0,20 M acetic acid with 35.0 ml of 0 10 M…

A: pH is used to determine the concentration of hydronium ion.

Q: 4. Explain how you determine the pH when 15 ml of 0.100 M HCI is added to 25 ml of 0.080 M NH3 (Kp =…

A: 4.pH can be calculated using Henderson - Hasselbach equation.

Q: When 35.0 mL of 0.200 M perchloric acid and 35.0 mL of 0.200 M potassium hypochlorite are combined,…

A: Given: perchloric acid=> Strong acid potassium hypochlorite => Conjugate base of HOCl (Strong…

Q: The most important way that the pH of the blood is kept relatively constant is а. 2+ by Ca O b. by a…

Q: A 80.0 mL sample of 0.0200 M HCI is titrated with 0.0400 M KOH solution. Calculate the pH after the…

A: The objective of this question is to calculate the pH at different stages of a titration between a…

Q: A buffer solution is composed of 0.12 M CH3OOH and 0.11 M CH3COONA а.) What is the pH of this…

A: NOTE: Please note according to our policy, we can only answer the first three subparts of a…

Q: 9. To prepare a basic buffer of pH=10 how many grams of NH,Cl would you add to 100 ml of 0.1 M NH¸OH…

A: The Henderson Hasselbalch equation for basic buffer is given as:

Q: Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the…

Q: 1. Calculate the pH: a) 0.005 n acetic acid solution; 2. What is the concentration of OH' ions in…

A: In this question, we have given some solutions. pH is a scale which measures the molar concentration…

Q: 5. Suppose 30.0 mL of 0.15 MKOH is added to 50.0 mL of 0.20 MHCIO. What will be the pH of the…

A: The question is based on the titrations. we are titrating a weak acid hypochlorus acid with a…

Q: When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt…

A: Given ionic salt is slightly soluble . Equilibrium constant = Ksp Ionic product = Qsp

Q: An acid solution is made by diluting 30.6 mL of 0.2360 HI to 1.000 L. 1. What is the pH of this…

A: pH measures the acidity of the solution. The concentration of hydronium ion. pH determined as…

Q: Calculate pH for a weak acid/strong base titration. Determine the pli during the titration of 65.0…

A: Since you have asked a question with the multiple subparts we will solve the 1st three subparts for…

Q: 13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is…

A: Sodium benzoate is a salt and HCl is an acid.

Q: 15.0 mL of the 1.0 M LIOH are added to 50.0 mL of 0.20 M H2SO4. What is the pH at this point in the…

A: Here, we have to find the pH of a titration when 15.0 mL of the 1.0 M LiOH are added to 50.0 mL of…

Q: Calculate the pH of a mixture that contains 0.25M of HCNO and 0.18 M of HC, H,O. The K, of HCNO is…

A: The ionization of weak acid is represented as:HA (aq) ⇌ H+ (aq) + A- (aq) Acid dissociation…

Q: umple of 0.393 M triethylamine, (C,H5),N, is titrated with 0.3 40.1 mL of nitric acid, the pH is es…

Q: Some K2SO, and KHSO, are dissolved in 250.0 mL of solution and the resulting pH is 6.88. Which is…

A: A buffer solution is a solution that is formed by the combination of a weak acid and its conjugate…

Q: A solution is prepared by combining 20 mL of 0.1M KH2PO4 and 60 mL of 0.1M Na2HPO4 in a 100 mL…

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M…

A: Answer :- Any organic acid is a weak acid .So here 4-chlorobenzoic acid is a weak acid. (a)Before…

Q: A 39.6 mL sample of a 0.270 M solution of NaCN is titrated by 0.330 M HCl. Kb for is CN- is…

A: Balanced Reaction NaCN + HCl --> NaCl + H2O NaCN is a salt of weak acid it reacts with HCl to…

Q: 1. A 0.36 M hydrocyanic acid (HCN) solution has a pH of 4.87. Give: (a) the balanced equation for…

Q: A titration is performed in which 0.10 M LIOH is added to a 200.0 mL sample of 0.40 M HF. What is…

A: HF is a weak acid it reacts with LiOH which is a strong base and gives fluoride ion. Now this…

Q: The 100. mL of buffer solution is 0.05 M in C2H3O2- and 0.10 M in HC2H302. What is the resulting pH…

A: 20.0 mL of 0.1 M HCl is added to 100 mL of buffer solution that is 0.05 M in C2H3O2- and 0.10 M in…

Q: Which of the following will raise the pH of a weak acid HA in aqueous solution? I. addition of HNO3…

A: (I) HNO3 is a strong acid and thus decreases the pH of the solution. Therefore, pH won’t increase on…

Q: When a solution is titrated with an base, an indicator (HIn) changes from yellow to blue (In). The…

A: Answer: An indicator is a chemical substance that indicates about the completion of titration by…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

8.
A 100. mL sample of 0.10 MHCI is mixed with 50. mL of 0.12 M NH.. What is the resulting pH? (K, for NH3 = 1.8 × 10--
3.07
10.93
1.57
12.43
1.40

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

5:48 PM Wed Nov 16 Today 5:48 PM 目。 oint when 15.0 ml. of o. 75% Calculate the pH of a titration at the point when 15.0 mL of 0.15 M NaOH is added to 30.0 mL of 0.20 M HNO3 Edit G ¯¯¯
Determine the pH during the titration of 62.0 mL of 0.342 M formic acid (K,- 1.8x104) by 0.342 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 93.0 mL of KOH
Calculate the pH when 4.0 mL of 2.0 M NaOH is added to the buffer solution containing 25mL of 1.0 M HC,H;O2 and 25mL of 1.0 M NaC2H;O2. Where, K, = 1.8m10-5. 4.75 5.03 4.50 5.25
Does the pH increase or decrease, and does it do so to a largeor small extent, with each of the following additions?(a) 5 drops of 0.1 M NaOH to 100 mL of 0.5 M acetate buffer(b) 5 drops of 0.1 M HCl to 100 mL of 0.5 M acetate buffer(c) 5 drops of 0.1 MNaOH to 100 mL of 0.5 MHCl(d) 5 drops of 0.1 MNaOH to distilled water
A 31.1 mL sample of a 0.190 M solution of NaCN is titrated by 0.230 M HCl. Kb for is CN- is 2.0x10^-5 Calculate the pH of the solution: 1. after the addition of 35.7 mL of 0.230 M HCl
What is the pH of the buffer solution that contains 3.2 g of NH,Cl in 250 ml of 0.13. M NH,? Is the final pH lower or higher than the pH of the D.13 M ammonia solution? (K, for ammonia is 1.8 x 10) pH of the buffer The final pH is than the pH of the 0.13M ammonia solution.
An buffer is prepared by combining 4 L of a 0.57 M X solution with 4 L of an 0.57 molar HXCI solution. The K, of X is 4.54 ×10-3. What is the pH of this buffer solution? Please express your answer to the second decimal place.
What quantity in moles of CHINH CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH: (Kb for CHINH₂ is 4.4 x 10) to make a buffer with a pH of 11.05?
Calculate the pH after 0.032 mole of NaOH is added to 1.00 L of each of the following solutions. a. 0.145 M HONH, (K = 1.1 × 10-) pH = b. 0.145 M HONH, Cl pH = c. pure H₂O pH = d. a mixture containing 0.145 M HONH₂ and 0.145 M HỌNH3 C1 pH =
Write the reaction that occurs and calculate the pH after... 15.0 mL of 0.100 M NaOH is added to 5.00 mL of 0.150 M HCl 25.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4) 80.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4)
A buffer solution is made up of 1.0 M NH3 and 1.0 M NH4CI. K₂NH3 - = 1.8 x 10-5 What is the pH when 20 mL of 0.60 M NaOH is added to 25. mL of the buffer? pH after base added [?] pH Enter
Give correct detailed Solution