Answered: Which one of the following salts, when…

Which one of the following salts, when dissolved in water, produces the solution with pH less then 7? (Circle all that applies) O CH,NH3l ONACIOA O UHSO, O KF

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 195IP: A certain acid, HA, has a vapor density of 5.11 g/L when in the gas phase at a temperature of 25C...

See similar textbooks

Related questions

Q: Identify the acid, base, conjugate acid and conjugate base in the following reactions: HF (aq) + H2O…

A: Note: As per our guidelines, we are supposed to answer only the first question (question number 1).…

Q: What are the pH and pOH of a solution of 2.0 M HI, which ionizes completely?

Q: What will be the Ka of an acid solution that is 0.012 % ionized when it is 0.20 M?

Q: The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution…

Q: Calculate the pH of a solution that is 9.00 % (w/w) NaOH and has a density of 1.098 g mL-1.

A: To calculate the pH of the given solution, first of all, we calculate the concentration of hydroxide…

Q: If CH3OONa is addddd to a solutiom of CH3COOH, i’d the pH of the acid going to increase or decrease

A: When the salt is added to the solution, then due to common ion effect, the solubility of an acid…

Q: 1. (Ph)₂CuLi THF 2. HBr ROOR Ph Br NH two steps

A: The question is based on the concept of organic synthesis. We need to synthesize the product using…

Q: This young child drinks a 1L bottle Cherry Coke (pH = 2.20). What is [H,O] in the bottle for this…

A: Hi there! Since you have posted multiple questions, we will answer the first question for you. If…

Q: CH3COOH + H2O --> H3O+ + CH3COO- Meaured pH of solution= 2.58 a) Calculate the [H3O+] at…

A: Here we have to determine hydronium ion concentration, acetate ion concentration and acetic acid…

Q: Carbonic acid CHe Cog) react in water to produce Hso" according to Pe cquation. cag) a) Determine…

A: Given reaction: H2CO3(aq) + H2O(l) ⇌ H3O+(aq) + HCO3-(aq) We have to determine the acid, base,…

Q: CH3COOH + H2O --> H3O+ + CH3COO- Meaured pH of solution= 2.58 10mL of 1M acetic acid a)…

Q: НО 3. PhMgBr (ex) 4. HCI, H2O НО НО Ph Ph

A: Grignard reagent is represented as RMgX where R is the any organic group. R may be alkyl, alkenyl,…

Q: 25.0 g sample of CH3COONa is completely dissolved in 500.0 mL of water and CH3COOH has an acid…

A: Given: Mass of CH3COONa = 25.0 g. And volume of solution = 500.0 mL = 0.500 L…

Q: 3. In an acidic solution the pH is (grcater than less than?) 7. In a basic solution the pH is…

A: According to Bronsted-Lowry concept, A base is a proton acceptor and an acid is a proton donor.…

Q: a cetain juice sample has [H+] = 1.0*10-4(exponet) a. what is the ph for this sample b. what is…

A: Equations for pH, pOH calculation:

Q: Solution A has a pH of 5.6. Solution B has a pH of 2.8. Which has a higher (H*] concentration? O…

Q: water are sketched below, as under cope so powerful individual atoms Could be seen. The same volume…

A: Acid give H+ ion in water. As a result water gets protonated and H3O+ forms in the solution. More…

Q: A 0.100 M solution of KNO2 has a pH that is a pH that is a) Less than 7 b) Equal to 7 c) More than…

A: pH = It is the measurement of H3O+ ion of a solution pH = -log [H3O+] For basic solution pH > 7…

Q: Font Paragraph Styles Complete the following table. [H,0*] [Or] Acidic pH pOH or Basic? a) 7.5 x…

Q: In a neutral solution, [H+] is the same as...

A: Answer - Neutral solution - A neutral solution can be defined as one where the concentration of…

Q: Ive decided that i stil want to have0.15L orage juice. I order to make it less acidic I need rasie…

A: Given:0.15 L orange juicepH 0.5Identify how much water is required to add to dilute juice to this…

Q: 5) What is the pH and pOH of a 6.2 x 10-5M NaOH solution? (Hint: this is a basic solution –…

Q: The pH of a basic solution is 11.39. What is [OH-]?

Q: nobasic acids. pH value than CH,SO,OH with

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: What are [H*], [OH-] and pH in a solution with a pOH of 12.11 15.

Q: Which of the following statements about acids is true? O All of the other statements are false O For…

A: The question is based on the concept of equilibrium. it involves calculation of hydronium ion…

Q: Balance the equation for Ht and OH-

A: This is a type of acid-base reaction which is also called neutralization reaction in an acid reacts…

Q: A solution that is 0.10 M in NH3 and 0.10 M in NH4Cl. The Kb of ammonia is 1.8x10-5. What is the…

A: Given, 0.1 M NH3 and 0.1 M NH4Cl

Q: Consider a solution which is 0.10M in CH3COOH and 0.20M in NaCH3COO. Choose ALL of the following…

A: The pH scale is logarithmic, indicating the hydrogen ion concentration in the solution. The method…

Q: Which of the following will form a buffer? O Bro with slowly added NaOH O KC2H3O2with slowly added…

Q: NH4Br neutral, basic, acidic, or cannot be determined?

A: NH4Br is acidic in nature which can be explained as:

Q: Predict the acid that has the smallest pK,. O They have the same relative acid strength O HCIO O…

A: The right answer is HClO3.

Q: Which of the following is the weakest acid? HOI HOCl HOBr Since they are all oxyacids,…

Q: 0.28 M LiOH [H+] [OH-] PH POH

A: pH power of hydrogen is the numerical measurement of acidity and alkanity of the solution. pH + pOH…

Q: Q3. Rank the strength of the following solutions based on the percent dissociation from weakest to…

A: The % dissociation data of the solution given is,

Q: nite the eacion for the acidic and busic Salts mchen It is dissolived M waier. Be sure 1o write The…

A: These reactions are the salt of Hydrolysis.

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

Chemistry
Please help me fast! Are choices 1 and 3
correct, That is what i think are correct
Which one of the following salts, when dissolved in water, produces the solution with pH less then
7?
(Circle all that applies)
OCH3NH3
O NACIO,
O UHSO,
O KF

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

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 a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
. Consider 0.25 M solutions of the following salts: NaCl. RbOC1, KI, Ba(ClO4),, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.
Write net ionic equations to explain the acidity or basicity of the various salts listed in Question 79.
For which of the following solutions must we consider the ionization of water when calculating the pH or pOH? (a) 3108M HNO3. (b) 0.10 g HCl in 1.0 L of solution. (c) 0.00080 g NaOH in 0.50 L of solution. (d) 1107M Ca(OH)2. (e) 0.0245 M KNO3