Analytical chemistry (1)Chapter-2-Analil chenDr. Maath T. AL-SaabExample 2-16Calculate the p-value for each ion in a solution that is 2.00 x 10-3 M in NaCl and 5.4 x 10M in HCl.

Concentration of NaCl = 2 × 10-3 M Concentration of HCl = 5.4 × 10-4 M P value For each ion…

Answered: Example 2-16 Calculate the p-value for…

Science

Chemistry

Example 2-16 Calculate the p-value for each ion in a solution that is 2.00 x 10-3 M in NaCl and 5.4 x 10 M in HCl.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 81E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?

See similar textbooks

Related questions

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Q-4- Explain in detail Two of the following. 1- Calculate the pH of 0.1 M ammonium chloride. pkb…

A: The question is based on the concept of chemical equilibrium and solutions. we have to calculate pH…

Q: • Calculate the pH of water sample with hydrogen ion concentration of 3.16 * 10-8 mols/L • Calculate…

A: pH = - log [H+]

Q: X Incorrect. 1) HNO3, H2SO4 2) Fe, H,O* 3) NaNO, HCI 4) CUCN Draw Your Solution Save for Later

A: Nitration of benzene is aromatic electrophilic substitution reaction where benzene ring acts as…

Q: EXAMPLE 9-8 Calculate the hydronium ion concentration in a solution that is 2.0 X 10-4 M in aniline…

A: The Equilibrium Reaction of hydrolysis of C6H5NH3+ given in the question is - C6H5NH3+ + H2O…

Q: What is [H30+] if I have a 0.1 M NaOH? This is the correct answer but i don't know how it was…

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

Q: 38. N2(g) + 3 Hz(g) following will occur > 2 NH,(g) if pressure is increased which of the a) nothing…

Q: Ihave some ammonia (20 M) dissociating in water. What is the pH? (4 sig fig) Kb=1.8E-05, x<<…

A: Given, Molarity of NH3 = 20M Kb = 1.8*10-5

Q: What is the percent ionization of a 0.35 M HCN solution (Ka = 5.8 x 10-10)? Answer in 2 Sf.

Q: What is the pH of a 100.0 mL 0.0500m HCN(aq) solution which is mixed with 5.00 mL 0.200 M KOH(aq) ?…

Q: 4) Find the [H3O*] of a 0.100 M HCN solution. Ka for HCN is 4.9 x 10-10

A: Record the given data, c = 0.100 M Ka = 4.9 x 10-10

Q: Criven ka = 2.5×10-9 Find the pH at a 0.724 M Savetion of the weak Jose bese Bro- ?

Q: Sodium hydroxide (NaOH) is a strong base. What is the [H+] and the [OH−] in a 0.001 M NaOH solution…

A: Given that - Molarity of NaOH Solution = 0.001 M Sodium hydroxide NaOH is a strong base, then…

Q: 6) What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5…

A: Given Kb for NH3 = 1.8 * 10-5. The two ionization reactions are as follows: NH4Cl -------> NH4+ +…

Q: Vhat is the concentration of X in a 0.150 M solution of the diprotic acid H,X? For H,X K, = 4.5 x106…

A: Which one of the following is correct answer

Q: Example 18-15: Calculate the concentration of all species in 0.100 M arsenic acid, H3ASO4, solution…

A: The ionization steps for arsenic acid is as follows: H3AsO4 ↔ H++H2AsO4-H2AsO4- ↔ H++HAsO42-HAsO42-…

Q: Find the percent ionization (?α) of a 0.25 M HNO2 solution. (Ka for HNO2 is 4.6 × 10-4) A) 1.2%…

A: The equilibrium constant is equal to the ratio of the concentration of the product to the…

Q: At 15°C water's Kw = 6.02 x 10-14. Write the equilibrium expression for water's self-ionization.…

Q: The Ka for benzoic acid is 6.5 10-5. Calculate the pH of a 0.10 M benzoic acid solution.

A: Benzoic acid is a weak acid so it will not completely be dissociated in its aqueous solution.…

Q: How is the total [H3O*] of a 0.050 M aqueous solution of sulfuric acid, H,S04, determined? O H2SO,…

A: The molarity of sulfuric acid is = 0.050 M Total H3O+ for this sulfuric acid is =?

Q: Calculate the Ka of a 0.44 M solution of H X that has a p O H of 12.1. Do not use scientific…

A: Given : Initial concentration of HA = 0.44 M And pOH of solution = 12.1 Since pH = 14 - pOH =>…

Q: Pre-lab question #3-4: Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2…

A: Given reaction is HNO2 + H2O <-> H3O+ + NO2-

Q: What is the pH of a 2.22 molar solution of NH4Cl(aq)? The Kb for NH3 is 2.7 x 10-5. Report answer…

Q: The following are equations that you might need to solve problem a-d: Kw = KaKь 14 = pka + pkb Kw =…

A: Given, Molarity of HCl = 0.100 M Volume of HCl = 25.0 mL Molarity of NaOH = 0.250 M The pH of the…

Q: Determine the concentration of hydroxide ions in 0.0648 M aqueous sodium hydroxide. Kw = 10-14

A: Given : [NaOH] = 0.0648 M Kw = 10-14 To determine :- Concentration of hydroxide ions i.e. [OH-]

Q: Determine [H3O+] of a 0.170 M solution of formic acid (Ka = 1.8 × 10-4). Express your answer using…

A: Given,

Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5 (Hint:…

A: Since NH4Cl is completely soluble in water, it is dissociated into NH4+(aq) and Cl-(aq). NH4+(aq) is…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

Q: Your answer is correct. The value of K for the C4H7O₂ ion is 6.7 x 10-10. What is the value of K₂…

Q: rite the expression for the Ka when HC₂H3O2 is dissolved in water 2H3O2 + H₂O C₂H3021 + H30+1 ][ Ka…

Q: - 10 The acid dissociation constant K, of boric acid (H,BO,) is 5.8 × 10 *°. a Calculate the pH of a…

A: Given - Dissociation constant =5.8×10-10 Concentration of boric acid =4.9 M To calculate - pH of 4.9…

Q: What is the pH of 0.62 M methylammonium bromide, CH3NH3Br? The Kb of CH3NH2 is 4.2 x 10-4. (value ±…

Q: SORTABLE LIST Que tion 12 Arrange these acids from weakest to strongest based on their K. value at…

Q: ve been struggling with these questions for my homework although I put my answers on them I have to…

Q: Lab Report #3-2-3: 0.1 M NaC2H3O2 solution, using the given pH data, write expression for equ…

A: The question is based on the concept of salt hydrolysis. we have to write expression of equilibrium…

Q: Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O…

Q: Overall: What is the pH of a 0.50 M solution of phosphoric acid? R I с E H3PO4 0.50 - X 0.50-x H₂PO4…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: In a solution with a pH of 7.0. What are the α1 and α0 values of the hypochlorous acid ? (For HOCl…

A: pH= -log [H+] [H+] = 10-7

Q: What is the percent ionization of a 0.15 M HOCl solution (Ka = 3.0 x 10-8)? Answer in 3 decimal…

A: Concept: HA ===== H+ + A- c(1-x) cx cx Let the…

Q: HCIO is a weak acid (K, = 4.0 × 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Use pH formula, used to calculate the pH of salt formed by weak acid and strong base to find the…

Q: 5. What is the pH when [H+] = 3.9 x 10-4? 6. What is the [H*]when pH = 9.86?

Q: For a 0.0448 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw =…

Q: What is the pH of a sol that is 0.15m in CH3coone and 0.20m in ch3cooh the ka of ch3cooh is 1.8x10-5

Q: For a 0.0411 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What…

Q: e proton concentrations of three solutions at 25 °C are given Basic Acidic Neutral Answer Bank [H]=…

A: If the pH of a solution is 7, then it is called a neutral solution. If the pH of a solution is more…

Q: Determine the pH of a .25 M CH3NH3Cl solution (Ka for CH3NH3+ = 2.3*10^-11)(Show the dissociation…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: molarity of the solution = 0.1 M The pH of the solution = 9.5

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Analytical chemistry (1)
Chapter-2-
Analil chen
Dr. Maath T. AL-Saab
Example 2-16
Calculate the p-value for each ion in a solution that is 2.00 x 10-3 M in NaCl and 5.4 x 10
M in HCl.

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

Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
C6H4NH₂COOH, para-aminobenzoic acid (PABA) is used in some sunscreens. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C6H4NH₂COO- in a 0.055 mol dm-³ solution of the acid. Ka-2.2 x 10-5
1. The Kb of HONH2 is 1.1 x 10-8. Calculate the pH and percent dissociation of a solution containing 0.100 M HONH2. а. b. Calculate the pH and percent dissociation of a mixture containing 0.100 MHONH2 and 0.100 M HONH3CI.
2-14. Calculate the p-value for each of the indicated ions in the following: (a) Na*, Cl, and OH- in a solution that is 0.0235 M in NaCl and 0.0503 M in NaOH. (b) Ht, Cl-, and Zn2+ in a solution that is 0.800 M in HCl and 0.101 M in ZnCl2. K+, OH-, and Fe(CN)- in a solution that is 3.79 X 10-7 M in K,Fe(CN), and 4.12 x 10-7 M (c) in KOH.
Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.
l Verizon LTE 7:55 PM O 4% C Question 8 of 8 Submit Which of the following accurately describes the major species in solution at point C on the titration curve for the titration of NH3 with HCl? pH C 7 В D mL H+ A) NH; and H* Tap here or pull up for additional resources A
Ex. 13-5. A 50.00-mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocresol green indicator. Calculate the molarity of the HCl. Ва(ОН)2 + 2HCІ- ВаCl, + 2H-0
Calculate the pH of a saturated solution of Mg(OH)2. Ksp [Mg(OH)2] = 1.8 × 10-¹1. Express your answer to two decimal places. View Available Hint(s) pH = Submit IVE ΑΣΦ ?
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
A Dashboard 101 Chem101 b Answered: At a particular temper X A aрp.101edu.co Question 3 of 23 Submit A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. НА(aq) H:O(1) H:O*(aq) A-(aq) + Initial (M) Change (M) Equilibrium (M) 2 RESET 0.1000 3.0 -3.0 0.030 -0.030 0.0030 -0.0030 0.0970 -0.0970 0.0097 -0.0097 + 10:34 PM P Type here to search 65°F Mostly sunny 10/31/2021
A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 ml ot a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONA). [Ka= 1.8 x 10-1 What is the new concentration of the conjugate base, CH3COO after buffering? 0.3385 0.2434 0.1172 0.2269 0.4287