Refer to the following equilbria and equilibrium constants and answer the following NH4+ (aq) + H2O NH3 (aq) + H3O + (aq) K a = 5.6 x 10 -10 HNO2 (aq) + H 2O NO2- (aq) + H3O + (aq) K a = 4.5 x 10 -4 Is an aqueous solution of NaNO 2 (sodium nitrite) acidic, basic or neutral? acidic neutral basic

Refer to the following equilbria and equilibrium constants and answer the following NH4+ (aq) + H2O NH3 (aq) + H3O + (aq) K a = 5.6 x 10 -10 HNO2 (aq) + H 2O NO2- (aq) + H3O + (aq) K a = 4.5 x 10 -4 Is an aqueous solution of NaNO 2 (sodium nitrite) acidic, basic or neutral? acidic neutral basic

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.103EP: Both ions in the salt ammonium cyanide (NH4CN) hydrolyze in aqueous solution. Explain why this...

See similar textbooks

Related questions

Q: What is the equilibrium concentration of H2C2O4 in a .542 M oxalic acid H2C2O4 solution? For oxylic…

Q: Consider the following reaction at equilibrium. 2 Cro42- (aq) + 2 H* (aq) = Cr20;2- (aq) + H20 (1)…

A: According to Le Chatelier’s principle the equilibrium of the reaction shifts if the concentration,…

Q: Suppose a 0.050M aqueous solution of oxalic acid (H2C2O4 ) is prepared. Calculate the equilibrium…

A: The acid dissociation constant of oxalic acid are Ka1 = 5.4 X 10-2 and Ka2 = 5.3 X 10-5 approx…

Q: What is Keg for the following reaction: HPO42 (aq) + H30*(aq) = H2PO4 (aq) + H2O(1) Some possibly…

Q: What is Keq for the following reaction: HPO42-(aq) + H3O+(aq) H2PO4-(aq) + H2O(l)Some possibly…

Q: For each of the following reactions, identify the acid and the base. Also indicate which acid-base…

A: 1. Fe3+ + 6 SCN– →[Fe(SCN)6]3– Lewis acid- Fe+3 Lewis base- SCN- According to this definition,…

Q: Arsenate (AsO43) is highly toxic as it is incorporated instead of phosphate in many biomolecules.…

A: THE REMOVAL OF 1ST H+ IS SHOWN IN THE FOLLOWING REACTION, H3AsO4aq⇌H2AsO4-aq+H+aq THE ICE TABLE IS…

Q: Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is…

A: The solution is as follows:

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: According to s principle, what would happen to the chemical balance of the ollowing equilibrium when…

A: Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the…

Q: In the following chemical equation indicate the reactant that is a Brønsted-Lowry acid HCN(aq) +…

A: Given, Chemical Reaction : HCN(aq) + H2O(l) ⇌ H3O+(aq) + CN-(aq)

Q: A mixture of hydrogen and iedine are in equilibrium with hydrogen iodide, as shown in the following…

A: The given reaction is,

Q: References] Obtain the equilibrium constant for the reaction HCN(aq) = H+ (aq) + CN¯(aq) From the…

Q: The following equation represents the dissociation of m-toluic acid in water. HC3H702(aq) + H20(1) =…

A: A reaction is said to be in equilibrium when the rate of forward reaction is equal to the rate of…

Q: What is the equilibrium concentration of H2C2O4 in a 0.542 M oxalic acid, H2C2O4, solution? For…

A: Acid dissociation Here we have a weak acid H2C2O4 which dissociates only to a small extent. H2C2O4…

Q: Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add…

A: According to Le-Chatelier's principle, the changes made in the system is counteracted by shifting…

Q: Calculate the equilibrium concentration of NO2 given [O2]eq = 0.060M, [H2O]eq = 0.0478M, and [NH3]eq…

A: Reversible reactions proceeding inside containers after reaching a specified stage becomes stagnant.…

Q: A solution of benzoic acid (HC7H5O2) is 14.2 percent ionized. Calculate the equilibrium…

A: The percent ionization is defined as the ratio of concentration of reactant dissociated and the…

Q: A monoprotic weak acid,HA, dissociates in water according to the reaction HA(aq)+H2O equilibrium…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: For the following reaction, respectively identify the Brønsted-Lowry acid and the conjugate acid.…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

A: Given reaction,

Q: Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate…

A: Here given pH is greater than 7 thus basic. Hence, heroine is a base. Now, using given pH to…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

Q: At 25 °C phosphoric acid, H3PO4, has the following equilibrium constants: Part A = 7.5 x 103 Ka K. -…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: According to the Brønsted-Lowry concept :- An acid is a proton donor A base is a proton acceptor

Q: Consider the reaction shown below: HSO4-1 (aq) + F-1 (aq) ⇋⇋ SO4-2(aq) + HF (aq)…

A: Bronsted-Lowery conjugate acid-base pair: The Bronsted-Lowery conjugate acid-base pair consists of…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: Phosphoric acid (H3PO4) is a weak acid naturally found in the body that supports kidney function and…

A: Given, Phosphoric acid (H3PO4) is a weak acid and it's Ka value is 6.9 * 10-3 at STP…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

A: Brønsted-Lowry acid is a substance which donates a proton i.e H+ ions in the reaction and…

Q: hydrocyanic acid (HCN) nitrous acid (HNO2) Ka=4.9×10−10 Ka=4.6×10−4 Use the information in the…

A: Given, Acid dissociation constant of HCN = Ka = 4.9 x 10-10 Acid dissociation constant of HNO2 =…

Q: The highlighted reactant acts as a... reaction (check all that apply) Brønsted-Lowry acid…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

Q: The ionization constant of a very weak acid, HA, is 1.9×109. Calculate the equilibrium…

Q: 9. Which equilibrium constant would be most relevant to the following system in equilibrium:…

A: Given: HC2H3O2 (aq) )⇌H(aq) ++C2H3O2-(aq) To find: relevant equilibrium constant.

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: Definition : A Bronsted-Lowry acid is a proton (H+ ) donor. A Bronsted-Lowry base is a proton (H+ )…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: Bronsted-Lowry acid-base theory: According to the Bronsted-Lowry acid-base theory, acid is a…

Q: 4-)

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: Write the equilibrium-constant expressions and obtain numerical values for each constant in (a) the…

A: Equilibrium constant gives the relation between the concentration of products and reactants when the…

Q: Arsenic acid is a triprotic acid whose ionization occurs according to the following reactions:…

Q: Phenol, C6H5OH, is a weak organic acid: C6H5OH(aq) = СâH5O¯(aq) + H+ (aq) Although somewhat toxic to…

Q: . Calculate the pH and all the equilibrium concentrations for the complete dissociation of a 5.0M…

A: Arsenic acid is a triprotic acid where H3AsO4 dissociates to H2AsO4- which then further dissociates…

Q: Calculate the equilibrium constant for the following reaction: H2SO3 (aq) =2 H+ (aq) + (SO3)2- (aq)…

Q: Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this…

Q: A 0.121 M solution of acetic acid has a pOH of 11.20. What is the K3 of acetic acid? Oa. 2.5 x 106…

A: Given: The concentration of acetic acid is 0.121 M The value of pOH is 11.20

Q: CoCl42-(aq) + 6H2O(l) >< Co(H2O)62+(aq) + 4Cl-(aq) 1) What was the original color of the…

A: Given data : Le Chatelier’s Principle: According to the principle that if a system is in chemical…

Q: Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate K…

Q: Achemist prepares a solution by dissolving the salt NaCIO2 in water. Calculate the value of the…

A: The salt given is NaClO2. The salt is made up of weak acid HClO2 and strong base NaOH. Hence the…

Question

Refer to the following equilbria and equilibrium constants and answer the following
NH₄⁺ (aq)  +     H₂O        NH₃ (aq)        +          H₃O ⁺ (aq)         K _a =    5.6 x 10 ^-10
HNO₂ (aq)  +   H ₂O          NO₂^- (aq)        +          H₃O ⁺ (aq)         K _a =    4.5 x 10 ^-4

Is an aqueous solution of NaNO ₂ (sodium nitrite) acidic, basic or neutral?

		acidic
		neutral
		basic

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
Both ions in the salt ammonium acetate (NH4C2H3O2) hydrolyze in aqueous solution. Explain why this hydrolysis produces a neutral solution rather than an acidic or basic solution.
Both ions in the salt ammonium cyanide (NH4CN) hydrolyze in aqueous solution. Explain why this hydrolysis produces a basic solution rather than an acidic solution.
Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K = 1.8 × 10–4. $$HCOOH(aq)+H2O(l)HCOO−(aq)+H3O+(aq) Calculate the equilibrium concentration of H3O+ in a 0.985 M solution. M
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. CN- + CH3COOH ⇌ HCN (aq) + CH3COO- Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase In this reaction: The formula for the conjugate _____acidbase of CN- is The formula for the conjugate _____acidbase of CH3COOH is
What is the equilibrium concentration of H2C2O4 in a .542 M oxalic acid H2C2O4 solution? For oxylic acid Ka1=6.1 x 10-2, Ka2= 5.1 x 10-5 a) 1.4 x 10-1 M b) 1.1 x 10-1 M c) 2.3 x 10-1 M d) 3.88 x 10-1 M e) 8.9 x 10-2 M
For the following chemical reaction, identify the acid, the base, and the conjugate acid and conjugate base. H2O(l) + ClO1-(aq) ⇄ HClO(aq) + OH-(aq) Brønsted-Lowry acid = Brønsted-Lowry base= HClO(aq) is the conjugate of .OH-(aq) is the conjugate of .
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCN (aq) + H2PO4- ⇌ CN- + H3PO4 (aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate (acid or base) of HCN is The formula for the conjugate (acid or base) of H2PO4- is
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. F- + H2CO3 (aq) ⇌ HF (aq) + HCO3- Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase In this reaction: The formula for the conjugate _____acidbase of F- is The formula for the conjugate _____acidbase of H2CO3 is
The following equilibrium constants have been dtermined for oxalic acid at 25°C: H2C2O4 (aq) = H+ (aq) + HC2O4- (aq) K1= 6.5 x 10-2 H+ (aq) + C2O42- (aq) = HC2O4- (aq) K2= 1.6 x 104 Calculate the equilibrium constant for the following reaction at the same temperature: H2C2O4 (aq) = 2H+ (aq) + C2O42- (aq) Kc= ?
1) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? 2) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from number 1? 3) Creating the concentrated acetic acid solution by dissolving liquid HOAc in water raises the temperature of the water by about 5 °C from room temperature. At 50 °C, do you expect the solution to contain more or less acetate ion OAc– than what you calculated in (2)? Why?
The ionization constant of a very weak acid, HA, is 1.6×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = _______ mol/L [A-] = __________ mol/L [HA] = _________ mol/L pH = ___________