pH values3.5SolutionsH20 (unboiled)H20 (boiled)7.0NaCl7.0NaC2H3029.1NHẠC14.5NaHCO39.5Na3PO411.9Na2CO311.0 Lab Report #4-2-2:0.1 M NH4CI solution, using the given pH data, write net-ionic equation forhydrolysis:NH4* + H20 + NH3¯ + H3O*NH4* + OH" +→ NH4OHNH4CI + H20 → NH3¯ + H3O* +Cl°

Salt hydrolysis :- The interaction of cation or anion or both of a salt to form an acidic or basic…

Answered: 0.1 M NH4CI solution, using the given…

0.1 M NH4CI solution, using the given pH data, write net-ionic equation for hydrolysis: NH4* + H20 + NH3¯ + H3O* NH4+ + OH" +→ NH4OH NH4CI + H20 → NH3¯ + H3O* +CI°

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: Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0443 M methylamine (CH, NH,)…

Q: Consider the following data on some weak acids and weak bases: Ka formula acetic acid HCH3CO₂ 1.8 x…

A: Given are the Ka and Kb value of weak acids and weak bases. More is the value of Ka and Kb, more…

Q: The K, of propanoic acid (C,H,COOH) is 1.34 × 10-³. Calculate the pH of the solution and the…

Q: A 100 cm³ sample of weak base 0.10 M methylamine, CH, NH,₂, (K₁ = 3.7 x 10), is titrated with 0.25 M…

A: The Kb of methylamine is given to be 3.7×10-4. Its pKb can be calculated as: pKb=-logKb…

Q: Calculate the pH of a solution containing 0.0460 M potassium hydrogen tartrate and 0.028 M…

Q: A diprotic acid, H, A, has acid dissociation constants of K 2.32 x 10 and K2 = 5.84 x 10-12.…

A: Hii there, As there are multiple question posted. we are answering first question. If you need…

Q: Q1a): Arrange the following 0.10 M aqueous solutions in order of increasing PH: Caso,, H,SO, NH,NO,…

A: (1a) The different types of salts formed by Acids and bases , if during the formation of salt,…

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

Q: A diprotic acid, H, A, has acid dissociation constants of Kal concentrations of H, A, HA, and A2- at…

Q: None

A: Step 1:Since H2A is a weak diprotic acid, it can donate two H+ ions. We will find the concentration…

Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…

Q: A 40.25 litre aqueous solution of a weak base, B-, has a concentration of 0.097 M. The Kb -value…

A: Kb = 5.00 x 10-12 [BOH] = 0.097 M

Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…

A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…

Q: Part A What is the pH of a 0.440 M ammonia solution?

A: [ NH3 ] = 0.44 M Kb = 1.8 × 10-5 pH = ?

Q: Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M…

A: The relation between pH and concentration of acid and its conjugate base is calculated using the…

Q: HF is considered a weak acid .Calculate the pH of an aqueous solution of 0.850 M HF (K₁ = 7.10 x…

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: Consider a 1.0-L solution that is initially 0.610 M NH3 and 0.750 M NH4Cl at 25 °C. What is the pH…

A: This is a basic buffer solution. pOH = pKb + log{[salt]/[base]} ...(1) Moles of NH3 = 0.610 Moles…

Q: 2.) Suppose in the following reaction we begin with 0.250M of HCN. What is the pH at equilibrium.…

A: HCN (aq) + H2O (l) ⇌ H3O+(aq) + CN- (aq) Ka=4.9 ×10-10 The concentration of HCN = 0.250 M

Q: Using the constant below, calculate the molar concentration (M) of acid H3O* in solution if the…

A: Kw is the water dissociation constant, and is given by :Kw = [ H3 O+] [OH-] Kw = 1 × 10-14[OH-] =…

Q: Aspirin (acetylsalicylic acid, HC₉H₇O₄) has a value of Ka equal to 3.3 × 10⁻⁴. What is the pH after…

Q: 0.85 g of hydrogen chloride (HCl) is dissolved in water to make 8.0 L of solution. What is the pH of…

A: Mass of HCl = 0.85 g Volume of solution = 8.0L

Q: Calculate the pH of 0.116 M NaC2H3O2 (sodium acetate) C2H3O2-(aq) + H2O(I) HC2H302(aq) + OH-(aq) Ka…

A: Ka of HC2H3O2 = 1.7510-5Molarity of NaC2H3O2 = 0.116 MKw = 1.010-14

Q: For a 8.21×102 M solution of H2Se, calculate both the pH and the Se2 ion concentration. State…

A: An acid when dissolved in water dissociate to form a conjugate base by releasing H+ ions. The extent…

Q: Can you please fill out the ice table and find the Ka

A: ICE tableKa Explanation:Step 1: ICE tableICEHC3H5O2 (aq)H2O (l)⇌H3O+ (aq)C3H5O2-…

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: The pH of a 8.3×10-2-M solution of phthalic acid (H2C8H4O4) is measured to be 2.03. Use this…

Q: If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.135 M, determine the carbonic…

Q: What is the pH of a 5.50x10-2 mol L-' ammonia solution? Express your answer numerically to two…

A: Weak base degree of dissociation (α) can be calculated by the given below formula α = KbCwhere…

Q: Determine the OH- and H+ concentration and calculate the pH, pOH of a solution that is 0.70 M NH3…

A: pH of a solution is a measure of acidity of a solution. pH less than 7 indicate that solution is…

Q: What is the pH of a 4.8 M pyridine solution that has Kp = 1.9 x 109? The equation for the…

Q: A diprotic acid, H, A, has acid dissociation constants of K₁1 = 4.76 x 10-4 and K₁2 = 3.59 x 10-12.…

Q: The base-dissociation constant (Kb) for this base is 1.7x109, If the pH of the solution is 9.15,…

Q: We can observe the common-ion effect in action by comparing how much a pure sample of acid…

A: Part-1: To calculate the pH of a solution having 0.100 M HIO solution given that the Ka of HIO is…

Q: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.0050 M, determine the…

Q: Calculate the pH and [H3O+] of a soln that is 0.050 M in HC2H3O2 and 0.10 M in NaC2H3O2. What…

A: Make an ICE table,Ka = [CH3COO-] [H3O+][CH3COOH]= (0.10+X) (X)(0.050-X)=1.80x10-5

Q: Oxalic acid, H2C2O4 , has acid dissociation constants of Ka1=5.90×10–2 and Ka2=6.40×10-5.Calculate…

A: Hii there, As there are multiple question posted. we are answering first question. If you need…

Q: Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, K,…

A: Given- HCN= 0.470 mole HC9H7O4 = 0.164 mole Volume of solution = 3.00 L Ka of HCN = 6.17 x 10-`10 Ka…

Q: Calculate the pH of a 0.384 M aqueous solution of hydrofluoric acid (HF, K₂ = 7.2x 10-4). pH =

A: It is based on the concept of acid and Base Here we are required to find the pH of A)0.384 M of…

Q: Arrange the following solution from lowest pH to highest pH: 0.75 M CH3COOH (K, = 1.8 x 10-5) 0.01 M…

Q: What is the pH of a solution prepared by adding 60.4 g ethylammonium chloride (C2H5NH3CI, 81.55…

A: As C2H5NH3Cl is salt of weak base and strong acid while C2H5NH2 is weak base so the resultant…

Q: This question is concerned with acid/base. The ionic product of water may be taken as 10-14…

A: Introduction: The Titration is provided a graph that is called titration curve which contains the…

Q: Consider a 0.25 M aqueous solution of the weak base, sodium acetate (NaCH3COO). The solution…

Q: Calculate the pH at 25 °C of a 0.82M solution of pyridinium chloride (C,H,NHCI). Note that pyridine…

A: Given , Concentration of C5H5NHCl= 0.82 M

Q: If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the…

A: Concentration of bicarbonate ion required can be calculated using Henderson hasselbalch equation for…

Q: Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215…

Q: Calculate the pH of a solution containing 0.70 M HC2H302 and 0.25 M NaczH302. The K, for HC,H;0, is…

A: Given :- Ka for HC2H3O2 = 1.8 × 10-5 concentration of HC2H3O2 = 0.70 M concentration of NaC2H3O2 =…

Q: The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to…

A: Since we know that if we dilute an strong acid solution it's pH will increase but if we dilute an…

Q: Use the References to access important values if Ka for acetylsalicylic acid (aspirin), HC,H7O4, is…

A: In this question, we will select the weakest acid. You can see the explanation 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

pH values
3.5
Solutions
H20 (unboiled)
H20 (boiled)
7.0
NaCl
7.0
NaC2H302
9.1
NHẠC1
4.5
NaHCO3
9.5
Na3PO4
11.9
Na2CO3
11.0

Lab Report #4-2-2:
0.1 M NH4CI solution, using the given pH data, write net-ionic equation for
hydrolysis:
NH4* + H20 + NH3¯ + H3O*
NH4* + OH" +→ NH4OH
NH4CI + H20 → NH3¯ + H3O* +Cl°

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

Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid 0.1 M KCI acid solution 0.1 M KCIO 0.1 M C6H5NH3Br 0.1 M NH4CI formula HCH3CO₂ 1.8 x 10-5 HCIO Ra Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 3.0 × 10 pH choose one -8 choose one choose one base choose one ✓ Ko name formula aniline C6H5NH₂ 4.3 × 10¯ - 10 ammonia NH3 1.8 × 10
Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for for pH to 2 decimal places. solution A B с [H₂O¹] 6.3 × 10 12 mol/L mol/L 0.44 mol/L PH 0 6.60 0 0 about 25 °C. X S ? [H₂O*] to to 2 significant digits, and your entries 圖山圆图

A solution is prepared at 25 °C that Is initlally 0.43M in dimethylamine ((CH, NH, a weak base with K, =5.4x10, and 0.15M in dimethylammonlum -4 and 0.15M In dimethylammonium bromide ((CH,),NH,Br) ((CH,) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. bгomide 2. pH Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privac hp
Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M HCl(aq) solution. Calculate the pH at 10.0 mL intervals of added HCl(aq), up to 50.0 mL, and plot the titration curve. Assume that the volumes are additive. Use pKb = 3.34 for methylamine.
Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (a) Write out the reaction that leads to this acidic pH.
Calculate the pH of a solution that is 3.67×10−53.67×10-5 M NH3 and 2.41×10−52.41×10-5 M NH4Cl.Kb=1.821.82 x 10−510-5NH4+1 (aq) + H2O(l) <----> NH3(aq) + H3O+1(aq)
For a 0.00533 M solution of sodium benzoate, NaC6H5CO2, do the following. Identify the major species (other than water) that has no effect on pH. Include charges and physical states in your answer. eTextbook and Media Balance the equilibrium reaction for the major species that does have an effect on pH. Include charges and physical states in your answer. +H,0(1)= Compute the pH of the solution. Ką of HC6H5CO2 is 6.3E-5. i
For a 5.55-102 M solution of H₂CHO calculate both the pH and the CH4O2 ion concentration. State symbols are not shown for water or the aqueous species in the reaction equations. HiệnHoDe+H2OHOHOH. Đó Ki-7,9×105 HC₂H₂O + H₂0H₂O + CH606² K₂21.6x10-12 pH = [CH₂O2)
For the diprotic weak acid H2A, Ka1-3.4x10-6 and Ka2=6.1×10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution? Express Ka1 in terms of x, and then show the simplified expression (when x is assumed to be negligible compared to to the initial concentration). Kal-A/B =C/D numerator A in complete expression: denominator B in complete expression: numerator C in simplified expression: denominator D in simplified expression: Also, give the numerical value of x using the appropriate approximation. What is the pH of the solution if you stopped here? X: pH:
The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2
If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.270 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.45. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 5.3 × 10-7 Show all calculations including equation(s) used. Provide your final answer to 3 decimal places.
Calculate K₂ or K from experimental data. The pH of a 9.7x10-2-M solution of phosphoric acid (H3PO4) is measured to be 1.65. Use this information to determine a value of K₂ for phosphoric acid. ? H3PO4(aq) + H₂O(1) H₂PO4 (aq) + H3O+ (aq) Ka =