MasteringChemistry: CHE154 S Xsession.masteringchemistry.com/myct/itemView?assic iew?assignmentProblemID=142965856&offset3DnextCHE154-H Gen Chem II Bronikowski S20Part AComplete the first column for H3O+] of Solutions 2 and 4.Express your answers to two significant figures separated by a comma.• View Available Hint(s)να ΑΣΦ[H3O+]2, [H3O*]4 =SubmitPart B Complete previous part(s)

Given information: For solution 2, [OH-] = 3.8 x 10-7 For solution 4, pH = 7.15

Answered: MasteringChemistry: CHE154 S X…

Science

Chemistry

MasteringChemistry: CHE154 S X session.masteringchemistry.com/myct/itemView?assic

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: The acid dissociation constant K of alloxanic acid (HC, H, N₂O₂) is 2.24 × 107. Calculate the pH of…

Q: (a) NH, + HCl= (c) HCO,- + OH- (b) CH,CH,O¯ + HCl= (d) CH,COO- + NH,+

A: Net ionic equation: The net ionic equation is a chemical equation for a reaction that involves only…

Q: Find the pH of 0.2 M ammonia solution (pka=9.74). 2) a) b) Find the initial concentration of the…

Q: Write a net ionic equation to show that hydrocyanic acid , HCN , behaves as an acid in water. + H20…

A: The answer to the following question is-

Q: Calculate the pH of the weak acid or base solutions. Report your calculated pH to 2 decimal places.…

Q: Cewer below some Ontions twen which of the electrolyes H₂ B03, Car0H/2HNO3, воз, салонта, NHued,…

Q: Question 26: Calculate the Ka and Kb of the following conjugate acids and bases to 2 significant…

A: Answer:If acid and base are conjugate of each-other then product of and will always be equal to…

Q: Amphetamine (C,H13N) is a weak base with a pKp of 4.2. Part A Calculate the pH of a solution…

A: 1-Phenylpropan-2-amine is amphetamine. Its molecular mass (M) is 135.23 g/mol Concentration of…

Q: 5) Given the following substances in order of increasing acid strength, (AOCT (99) (HC2H302 (99)k…

Q: If in a solution [H,01-10 [OH ], what is the pH of the solution?

A: Given that : [H3O+] = 10 [OH-] We need to determine pH of this solution.

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: 6. Find Ka and Kb of each of the following amphiprotic anions and determine if they act as an acid…

A: The amphoteric ions are the ions which can acts as both the acid and base in aqueous solution. In…

Q: 1)For the following acid/base reactions, draw the products and indicate the equilibrium position.…

Q: Enough base was added to an amount of water to produce an aqueous solution with [OH-] = 2.4 x 10-5.…

A: Given, Concentration of Hydroxide ion = [OH-] = 2.4 × 10-5 M Concentration hydronium ion = [H3O+] =…

Q: Use Le Châtelier's Principle and the following table to predict the change in enthalpy and sign for…

A: The correct option with explanation is given below:

Q: now.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics]…

Q: a solution that is 0.20 M in HCHO2 and 0.12 M in NaCHO2 (Ka (HCHO₂) = 1.8 × 10-4) Express your…

Q: What mass of NaOH(s) must be added to 1.0 L of 0.045 M NH3 to ensure that the percent ionization of…

A: The reaction happening is as follow: NH3 + H2O ----> NH4OH…

Q: Ka for hypochlorous acid, HCIO, is 3.50x108 Ka for hydrocyanic acid, HCN, is 4.00x10-10 Ka for…

A: The species formed after the removal of proton from acid is known as conjugate base of the acid.This…

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula formula…

A: The solutions given are of KCl, CH3NH3Cl, NaCN and C2H5NH3Br.

Q: tô těst the acid-base properties of anions in a controlled experiment, which of e solids in the…

A: Given that the acid- base properties of anion

Q: H3O+ is the acid and CH3 CH2OH is the base. Express your answers as a chemical expression. ΑΣφ ?…

A: Acids are the species which can donate proton whereas base can abstract proton. Here we need to…

Q: (a) Compare between Electron ionization (EI) and Chemical ionization methods.

A: Interpretation- We have to compare between electron ionization (EI) and Chemical ionization methods…

Q: Explain why KNO3 is a suitable salt to be used in salt bridge.

Q: Xeon difluoride, XeF2, can act as a Lewis base toward metal cations such as Ag+ or Cd2+. Do you…

A: The electron donation towards Ag+ or Cd+2 happens via the electron of Xe, not the electron of F.…

Q: (d) calculate the pH of 0.015 M methylammonium nitrate ( CH3NH3*)(NO;) dissolved in water.

Q: 17.8. Part A A 0.190 M solution of a weak acid (HA) has a pH of 2.91. Calculate the acid ionization…

Q: Show and explain the relationship between pH, pOH, [H+], and [OH-], Kw, Ka, and Kb.

A: All the given terms are related to acidic and basic strength.

Q: For the following five reactions: (i) Cl− + AlCl3 → AlCl4− (ii) (CH3)3N + HCl → (CH3)3NHCl (iii)…

A: The reactions given are, (i) Cl− + AlCl3 → AlCl4−(ii) (CH3)3N + HCl → (CH3)3NHCl(iii) OH− + H3O+ →…

Q: Which acid is stronger: HF (Ka = 3.5×10−4) or HClO (Ka = 2.9×10−8)? How do you know

A: Ans

Q: Calculate [H3O+] and [OH-] for a solution that is 0.050 mol L¹ in HBr and 0.017 mol L-¹ in HNO3.…

A: for the given solution, we have to calculate [H3O+] and [OH-]

Q: In the following chemical reaction identify the acid. Don't worry about the charges and no need for…

A: Given [Al(H2O)6]3+ + 3H2O → [AI(H2O)3(OH)3]2+ + 3H3O+

Q: Identify the Lewis base in the following reaction: S*O_{2}(g) + H_{2}*O(1) -> H_{2}*S*O_{3}(aq)

A: The question is concept of chemical reactions. we need to identify Lewis base in the given reaction.

Q: The Ka value for hypochlorous acid (HClO) is 3x10-8 at 25 ºC. What is the ionization percentage of…

A: The concentration of hydrogen ions released by HClO at equilibrium can e determined as follows: H+ =…

Q: b) Show the reaction of HI, considered as a Bronsted- Lowry acid, with ethanol (C,H,OH).

Q: The pH of a 0.75M solution of 3-hydroxypropanoic acid (HC₂H5O₂) is measured to be 2.32. Calculate…

Q: Phenylephrine is a nasal decongestant and is the active ingredient in Sudafed, which contains…

A: #A: Since HCl is a strong acid, the H+(aq) of HCl will be accepted by the atoms of PE which is basic…

Q: Quien below Some ontions & which of the tectrolyes NHued, NH₂OH, CH3Cook, weak H₂B03, CarOHT₂, HNO3,…

A: Electrolytes : These are chemical species which conduct electricity when dissolved in…

Q: 4. What would the hydroxide ion concentration be if the hydrogen ion concentration was 1 x 10 M?

A: Given data for this, [H+] = 1×10-5 M

Q: uestion 10 of 15 For the diprotic weak acid H2A, Kal = 2.2 × 10 ° and K2 = 5.2 x 10-9. What is the…

Q: Part A Calculate the [H₂O+] of a 0.897 mol L¹ citric acid (H, C6Hs O7) solution. (Kai = 7.4 x 104,…

A: Since you have posted multiple questions, we will provide the solution only for the two sub-parts of…

Q: The perecent of ionization of 0.2 MNH3 is (Hint K, = 0.000018) (Write your answer to 1 d.p e.g 1.2)

A: Percentage ionisation can be calculated as follows

Q: Considering that [H3O +] 2 + ka [H3O +] - kaCHA = 0 is equivalent to 3x2 + 6x - 2 = 0, indicate the…

A: Recall the given expression H3O+2 + KaH3O+-KaCHA=0 .......(1) The above equation is equivalent…

Q: How many grams of K2A (M. W. 166.22) should be added to 15.0 mL of 0.200 M HCIO4 to give a pH of…

A: ANSWER:-the pH is 4.70the acidity constants H2A are 5.36×10-2 and 5.42×10-5 Here,the reaction is…

Q: Write the formula of the conjugate base of C6H5NH2.

A: Bronsted -Lowry concept: An acid is a substance which can donate proton and base is a substance…

Q: [он] - 7 х 105 м pH = 4.2 [н]3 1 х 1010М РОН 3 6.7

A: Basic solution which have pH greater than 7. Acidic solution has pH solution less than 7. And…

Q: Calculate the concentration (M) of the anion Z2- for a 0.100 M solution of H2Z given the acid…

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

Question

MasteringChemistry: CHE154 S X
session.masteringchemistry.com/myct/itemView?assic
<CHE154 S20 Ch17 Sec5-6
Exercise 17.52 Enhanced with Feedback and Hints
MISSED THIS? Read Section 17.5 (Pages 740 - 744);
Watch IWE 17.3.
Complete the following table. (All solutions are at 25 °C.)
Solution H3O+]
[ОН ]
Acidic, basic,
or neutral
pH
3.5 x 10-3
3.8 x 10-7
1.8 x 10-9
4.
7.15
Part B
Part C
2.
3.

iew?assignmentProblemID=142965856&offset3Dnext
CHE154-H Gen Chem II Bronikowski S20
Part A
Complete the first column for H3O+] of Solutions 2 and 4.
Express your answers to two significant figures separated by a comma.
• View Available Hint(s)
να ΑΣΦ
[H3O+]2, [H3O*]4 =
Submit
Part B Complete previous part(s)

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

9 eq 4 20 E D Write the equations that represent the first and second lonization steps for tellurous acid (H₂TeO3) in water. (Use H3O+ Instead of H+.) First ionization step: C Second lonization step: $ Submit Answer 4 000 000 F4 R + H₂0(1) = F + H₂0(1) = | V % 5 [Review Topics] [References) Use the References to access important values if needed for this question. T Retry Entire Group 9 more group attempts remaining F5 G Cengage Learning Cengage Technical Support 6 B FO + MacBook Air Y + H & 7 N F7 U * 8 J ➤11 FB 1 M I -o 9 K O S.P d ) O L F10 P 4) F11 Previous Next> + 11 alt ? Save and Exit F12 11 delete
Explain why NaOH, NaHCO3 and Na2CO3 cannot exist together and examine each case by writing related reactions.
How do you explain the pattern/trend in the distance between the anion of an acid and H3O+? The acid strength is HCl > HNO3 > HF > HOCl, but I don't understand why the lengths vary like this. Or does it have to do with electronegativity? If it does have to do with electronegativity, why doesn't HF have the shortest length? Or is it because OCl- is more elctronegatvie than F-? Also, does an acid's strength decrease/increase with increasing electronegativity of its conjugate base? When looking at the trend, HI is stronger than HBr, which is stronger than HCl. However, HClO4 is stronger than all of these acids, which I don't understand why.
Enter an equation to show how HC204 can act as a base with HS acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. 0 xa ΑΣΦ Xh Pu Part B a b A chemical reaction does not occur for this question. Y Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining ΑΣΦ Enter an equation to show how HC₂04 can act as an acid with HS acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer. ? X A chemical reaction does not occur for this question.
Calculate the pH of a 0.10 mol L- solution of HCl. Express your answer numerically using two decimal places. • View Available Hint(s) ΑΣφ ? pH =
0.75 mg/L of hypochlorous acid (HOCl) is added to water at 25 C. The pH of the water is adjusted to 6.54. What is the molar ratio of hypochlorite ion (OCl-) to hypochlorous acid? Show your work. Given: HOCL ↔ H+ + OCl- ; Ka = 10-7.54; MW’s: H = 1; O = 16; Cl = 35.45
What molar concentration of hydrazine, N2 H4 (Kb = 1.7 x 10 -6 ) yields a solution with a pH of10.64?
Choose the correct answer from among the alternatives; To make the sentence true: hydrocyanic acid HCN, the ionization constant Kaq = A) [Ka = [H3O +] / [H2O] [HCN B) [Ka = [H3O +] [CN-] / [HCN C)[Ka = [CN-] / [H2O] [HCN D) [Ka = [CN-] / [H2O
Please help me, double check your answers as previous tutors got it wrong.
Q6\ How to prepare(10 MI)of 0.2 N of NaoH, m. wt NaOH =40
Initial pH 2, 4 ,6 ,8, 10 and 12 Final pH 1.98, 4.47 , 6.56 , 7.01 , 7.02 and 11.06 Draw/determine the Point of zero charge
What concentration of acetic acid would produce an aqueous solution with a pH = 3.275? (Ka for HC2H3O2 = 1.76 x 105)