What is a compound that can donate a proton called? a. Bronsted-Lowry acid b. Bronsted-Lowry base...
Question:
What is a compound that can donate a proton called?
a. Bronsted-Lowry acid
b. Bronsted-Lowry base
c. Lewis acid
d. Lewis base
Bronsted-Lowry and Lewis Acid-Base:
The Bronsted-Lowry and Lewis definition of acid-base uses two different concepts: acceptance/donation of unshared pair of electrons and protons. For example, nitric acid is a Bronsted-Lowry acid and aluminum chloride is a Lewis acid.
Answer and Explanation: 1
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View this answerA compound that can donate a proton is called a Bronsted-Lowry acid.
For example, {eq}\rm HCl {/eq} is a Bronsted-Lowry acid as it dissociates...
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Bronsted-Lowry Acid: Definition & Examples
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Chapter 16 / Lesson 17
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Learn about Bronsted-Lowry acid. Understand the Bronsted-Lowry acid definition, the mechanisms, and see Bronsted-Lowry acid and base conjugate examples.
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- Which of the following is an electron pair acceptor? a. Arrhenius acid b. Arrhenius base c. Bronsted-Lowry acid d. Bronsted-Lowry base e. Lewis acid f. Lewis base
- Which acts as a Lewis acid but neither Arrhenius nor Bronsted-Lowry? a. H2CO3 b. HCO3- c. BF3 d. HClO3
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- Which of the following is a Bronsted-Lowry base but not a Lewis base? a) H_2O b) CO_3^{-2} c) CN^- d) NH_3 e) all choices are both a B/L and Lewis base.
- What is a Bronsted-Lowry base compound? Give some examples.
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- Classify each of the compounds NaH, BeH_2, BH_3, CH_4, NH_3, H_2O, and HF as a Bronsted-Lowry base, a Bronsted- Lowry acid, or neither.
- According to the Bronsted-Lowry model, an acid is a "proton donor" and a base is a "proton acceptor". Explain.
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- (a) Identify the reactant that is a Bronsted - Lowry acid in the following reaction: CO_3^{2-} (aq) + H_2O (l) to HCO_3^-. (aq) + OH^- (aq) Express your answer as a chemical formula. (b) Identify the reactant that is a Bronsted - Lowry acid in the followi
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- Define the following terms: Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, Lewis base.
- Which of the following is a Bronsted Lowry base? (a)Cl^{ -} (b)HNO_3 (c)NH_4^{+} (d)HNO_3
- Which of the following is a Bronsted- Lowry base? Cl2 HCN NH3 CH4
- Identify the Bronsted-Lowry acid and base in the reaction below: K O H + H B r H 2 O + K B r
- CH_3CH_2OCH_2CH_3 is best classified as a ______. A) Bronsted-Lowry acid. B) Lewis acid. C) Bronsted-Lowry base. D) Lewis base. E) Both C & D.
- What substance is acting as the Bronsted-Lowry base in the forward reaction below? H2O + HCl = H3O+ + Cl-
- Which pair below cannot have a Bronsted-Lowry acid base reaction between them? a. OH- and NH b. PO43- and ClO- c. HCO3- and SO32- d. HClO4 and HNO2 e. HSO4- and HCl
- How is a species that donates electrons classified? a. Lewis base b. Lewis acid c. Bronsted-Lowry acid d. Bronsted-Lowry base
- What are the two Bronsted-Lowry acids in the following: H2S+H2O <----> HS-+H3O+
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- Tell if the given compound acts as a Lewis base, a Bronsted-Lowry base, both, or neither.
- CH3CH20CH2CH3, is best classified as A. Bronsted-Lowry acid B. Lewis acid C. Bronsted-Lowry base D. Lewis base E. Both C& D
- Classify the following substances as a Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, and/or Lewis base. HCl, BF_3, CCl_3, -H CH_2O, CH_3Cl -OCH_3 , NH_3
- Classify each of these compounds as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. H2SO4, HF, HNO2, (CH3)3N, C2H5NH2, NH3, KCl, CHCl3.
- HNO3 (aq) + H2O (l) \rightarrow H3O+ (aq) + NO3- (aq) Identify the reactant that is a Bronsted- Lowry Acid and the reactant that is a Bronsted- Lowry Base in the reaction.
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- Bronsted and Lowry defined an acid as a(n) (a) electron donor. (b) electron acceptor. (c) proton donor. (d) proton acceptor.
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- Which of the following is both an Arrhenius and Bronsted-Lowry base? a. HCOOH(aq) b. NH4OH(aq) c. HCl(g) d. NH3(g)
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- Which of the following can act as a Bronsted-Lowry acid or base in water? (a) HCO_3^- (aq) (b) OH^- (aq) (c) HI (aq) (d) NH_2^ (aq)
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- For each reaction, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. a. HBr(aq)+H_2O(l) \rightarrow H_3O^+(aq)+Br^-(aq) b. NH_3(aq)+H_2O(l) \rightleftharpoons NH^{+4}(aq)+OH^-(aq) c. HNO_3(aq)+H_2O(l
- What is the difference between a Bronsted Lowry acid and a Lewis acid?
- For the following, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. HBr (aq) + H_2O (l) to H_3O^+ + Br^- (aq)
- For the following, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. HI(aq) + H_2O to H_3O^+(aq)+I^-(aq)
- Which one of the following can behave either as a Bronsted-Lowry acid or a Bronsted-Lowry base in an aqueous solution reaction? a. HSO_4^-. b. HI. c. CH_4. d. H_3PO_4.
- If a substance is an Arrhenius base, (a) is it necessarily a Bronsted-Lowry base? (b) Is it necessarily a Lewis base? Explain.
- Perchloric acid is either a Bronsted-Lowry acid or a Bronsted-Lowry base. If it is an acid, what is its conjugate base? On the other hand, if it is a base what is its conjugate acid?
- What is the conjugate acid of the Bronsted-Lowry base HAsO42-?
- What is the conjugate acid of the Bronsted-Lowry base CH3NH2?
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- A Bronsted-Lowry base is a compound that does which of the following? a. accepts a hydrogen ion b. supplies a peroxide ion c. supplies a hydride ion d. accepts an amide ion e. accepts a hydroxide ion
- What is the conjugate base of the Bronsted-Lowry acid HPO42-?
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- Complete the sentence: A Bronsted-Lowry base: a. is a hydrogen ion acceptor. b. dissociates to produce a hydroxide ion in aqueous solution. c. can accept a lone pair of electrons. d. can donate a lone pair of electrons. e. is a hydrogen ion donor.
- Complete the sentence: A Bronsted-Lowry acid: a. is a hydrogen ion acceptor. b. dissociates to produce a hydroxide ion in aqueous solution. c. can accept a lone pair of electrons. d. can donate a lone pair of electrons. e. is a hydrogen ion donor.
- Define a Bronsted-Lowry base.
- Which of the following is NOT a Bronsted-Lowry acid? a. H_2O b. CH_3CO_2H c. (CH_3)_3N d. NH_4^+
- Which of the following cannot act as a Bronsted-Lowry acid? (a) NH4+ (b) NO3- (c) HCl (d) HC2H3O2 (e) H3PO4
- Identify each reactant and product in the given chemical reaction as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither. Arrange the species in the given reaction as conjugate acid-base pairs. HNO2+H2O--H3O+ +NO2-
- Identify the Bronsted-Lowry acid and base conjugate pairs for the equation: OH^- + HPO_4^{2-} to H_2O + PO_4^{3-}
- Identify the Bronsted-Lowry acid in the following reaction. H 2 O ( l ) + C O 2 3 ( a q ) H C O 3 ( a q ) + O H ( a q ) (a) H 2 O (b) C O 2 3 (c) H C O 3 (d) O H (e) H 2 C O 3
- In the Bronsted-Lowry system, a base is defined as: (a) a proton donor. (b) a hydroxide donor. (c) an electron-pair acceptor. (d) a water-former. (e) a proton acceptor.
- What is the conjugate base of the Bronsted-Lowry acid HCOOH?
- Which of the following is not a Bronsted-Lowry acid? a. H2CO3 b. HCO3- c. CO32- d. H2O e. H3O+
- Is NH3 classified as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither? Explain.
- Is HI classified as a Bronsted-Lowry acid, a Bronsted-Lowry base, or neither? Explain.
- Identify each of the following species as a Bronsted-Lowry acid, base, or both. a) HI b) CH3COO- c) H2PO4- d) HSO4-
- How might one describe a base according to the Bronsted-Lowry theory? A. a proton donor B. produces OH- in solution C. a proton acceptor D. produces H+ in solution E. none of the above
- What substance is acting as the Bronsted-Lowry base in the forward reaction below? H_2O + NH_3 yields NH_4^+ + OH^-.
- The compound BF3 can be described as a(n): a. Arrhenius acid b. Bronsted-Lowry acid c. Lewis acid d. Lewis base
- In the reaction below, identify the Bronsted Lowry acid, base, conjugate acid and conjugate base. CO_3^{2-} + H_2O to HCO_3^- + OH^-
- Identify the Bronsted-Lowry acid in the following reaction. H_2O (l) + HCO_3^{1-} (aq) to H_3O^+ (aq) + CO_3^{2-} (aq).
- Which of the following species acts as a Bronsted-Lowry acid in water?
- In the reaction below, identify the Bronsted Lowry acid, base, conjugate acid and conjugate base. HSO_4^- + OH^- to SO_4^{2-} + H_2O
- Using the Bronsted-Lowry concept of acids and bases, identify the Bronsted-Lowry acid and base in each of the following reactions: H2PO3?(aq)+H2O(l)-->H3PO3(aq)+OH?(aq) (CH3)3N(g)+BCl3(g)-->(CH3)3NB
- Why can't NH_3 donate a proton and act as a Bronsted-Lowry acid?
- How is a species that can accept electrons classified? a. Lewis base b. Lewis acid c. Bronsted-Lowry acid d. Bronsted-Lowry base
- Identify the Bronsted/Lowry acids in the following reaction: HF + HPO4 2 F + H2PO4 -
- Classify each of the following as either a Bronsted-Lowry acid, base, or amphiprotic. (a) H 2 S O 4 (b) H S O 4 (c) S O 2 4
- Identify which of the following species can be Bronsted-Lowry bases. Indicate Yes or No. (a) I^- (aq) b) HCO_3^- (aq)
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