Draw out a chemical reaction between HCl and NH3. Indicate Bronsted acids and bases; what makes...
Draw out a chemical reaction between HCl and NH3. Indicate Bronsted acids and bases; what makes a chemical a Bronsted acid or base?
Homework Answers
Bronsted Lowry concept of Acid & Base ;- According to this concept acid is a proton donor & base is a proton acceptor.
It can be define as -
Acid + Base <-----> Conjugate base + Conjugate acid
(This is the general Equation which helps us to understand the concept of Bronsted Lowry Concept of acid and base)
Acid lose a proton & becomes conjugate base &
Base accept a proton & becomes conjugate acid.
Now,
HCl + NH3 <-------> Cl- + NH4+
Where HCl = acid ; NH3 = Base ; Cl- conjugate base ; NH4+ = conjugate acid.
HCl is a acid because it is a proton donor & further it donate/lose a proton and becomes conjugate base Cl-.
NH3 is a base because it is a proton acceptor & further it accept a proton and becomes conjugate acid NH4+.
Add Answer to:
Draw out a chemical reaction between HCl and NH3.
Indicate Bronsted acids and bases; what makes...
Identifying Bronsted Lowry acids and bases For each chemical reaction in the table below, decide whether...
Identifying Bronsted Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Bronsted-Lowry acid, a Brensted-Lowry base, or nether highlighted reactant reaction Bronsted Lowry Bronsted Lowry ither acid base + OH (ag)- Br (aq) +H,O HBr(aa) C Br (ag)+H.Om HBr(ag)+ OH (ag) Br (ag)+ H,Oc) HBr(ag) + OH (a) H,O HBrag)+OH (og) Br (ag)+ 1
Based on your understanding of Bronsted acids and bases - what is the role of water...
Based on your understanding of Bronsted acids and bases - what is the role of water molecules in the auto-ionization of water reaction shown below? H2O(l) + H2O(1) ► OH(aq) + H30*(aq) H2O molecules are only functioning as a Bronsted acid in this reaction H2O molecules are functioning as both a Bronsted acid and base in this reaction H2O is not functioning as a Bronsted acid or a base, it is the solvent / liquid O H2O molecules are only...
JU U NN ENZVAYC-XURXYM2368qJhw3sVPMJc4p33sdtyEbxd. y Genesis ACOS AND LASES Identifying Bronsted-Lowry acids and bases For each...
JU U NN ENZVAYC-XURXYM2368qJhw3sVPMJc4p33sdtyEbxd. y Genesis ACOS AND LASES Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Bransted-Lowry base, or neither reaction highlighted reactant Bronsted-Lowry Bronsted-Lowry acid base neither H, SO (aq) + NH3(09) - HSO (aq) + NH HSO (aq) + NH(aq) → H, SO. aq) + NH, (aq) H, SO (aq) + NH3(aq) - HSO (aq) + NH HSO (aq) + NH (0)...
#2 & 3 Identify the following species in water, as Bronsted Acids [A] or Bronsted Bases...
#2 & 3
Identify the following species in water, as Bronsted Acids [A] or Bronsted Bases [B]: H_3O^+; H_2SO_4; OH^-; HCN; CH_3COOH; CH_3NH_2 WRITE NET Ionic Equations for the reactions of H_2PO_4^-, an amphiprotic ion, with aqueous solutions of HCl KOH Give the conjugate base for each of the following acids: HI HSO_4^- H_2CO_3 C_2H_5NH_3^+ Give the conjugate acid for each of the following bases: NH_3 O^2- H_2O PO_4^3- Identify the conjugate acid-base pairs in each of the following reactions:...
Acids and bases: Part I Consider the following reactions: (a) 2 NH3 + Ag+ → [Ag(NH3)2]+...
Acids and bases: Part I Consider the following reactions: (a) 2 NH3 + Ag+ → [Ag(NH3)2]+ (b) NH4+ + CO32- → NH3 + HCO3- (c) 2 HBr + Ca(OH)2 → CaBr2 + 2 H2O Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true. Choices: a)Lewis-base b)Bronsted-Lowry and Lewis Base c) Lewis acid d) Arrhenius, Bronsted-Lowry, and Lewis acid...
answer all parts clear and accurate Indicate whether the following species are Arrhenius acids or bases...
answer all parts clear and accurate
Indicate whether the following species are Arrhenius acids or bases and/or Bronsted-Lowry acids or bases: 1. Both Arrhenius and Bronsted acid 2. Bronsted base NH2 3. Bronsted acid HCIO 4. Arrhenius acid 5. Arrhenius base 6. Both Arrhenius and Bronsted base
Write equations for the reaction of each of the following Brønsted-Lowry acids and bases. Identify the...
Write equations for the reaction of each of the following Brønsted-Lowry acids and bases. Identify the conjugated acids and bases. a. Acid: H20; base: NH3 b. Acid: NH4+, base: OH- c. Acid: HSO4; base: H2O d. Acid: HCl; base: H2PO4 6.4
Identify the Bronsted acids and bases in the following equation (A-Bronsted acid, B = Bronsted base):...
Identify the Bronsted acids and bases in the following equation (A-Bronsted acid, B = Bronsted base): CH3OH OH H2O CH30 a) A BBA b) BA BA c) A BA B d) BAA B
6. There are two major theories of acids and bases in aqueous solutions: Arrhenius and Bronsted....
6. There are two major theories of acids and bases in aqueous solutions: Arrhenius and Bronsted. a) In your own words, briefly explain the main difference between the two theories of acids and bases b) Which theory do you think is the most useful in chemistry? Explain your choice. c) Which of the following is an Arrhenius acid? A) H2SO4: B) LiOH; C) NH2CH3; D) CH3CH3; E) More than one of these is an Arrhenius acid. d) Which of the...
In general theory, are the conjugate acids and bases of a bronsted lowry acid-base reaction water...
In general theory, are the conjugate acids and bases of a bronsted lowry acid-base reaction water soluble? In my head, I was thinking that since the conjugates are charged, they're able to interact as salts in water. Is this true to some extent?
Identifying Bronsted Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Bronsted-Lowry acid, a Brensted-Lowry base, or nether highlighted reactant reaction Bronsted Lowry Bronsted Lowry ither acid base + OH (ag)- Br (aq) +H,O HBr(aa) C Br (ag)+H.Om HBr(ag)+ OH (ag) Br (ag)+ H,Oc) HBr(ag) + OH (a) H,O HBrag)+OH (og) Br (ag)+ 1
Based on your understanding of Bronsted acids and bases - what is the role of water molecules in the auto-ionization of water reaction shown below? H2O(l) + H2O(1) ► OH(aq) + H30*(aq) H2O molecules are only functioning as a Bronsted acid in this reaction H2O molecules are functioning as both a Bronsted acid and base in this reaction H2O is not functioning as a Bronsted acid or a base, it is the solvent / liquid O H2O molecules are only...
JU U NN ENZVAYC-XURXYM2368qJhw3sVPMJc4p33sdtyEbxd. y Genesis ACOS AND LASES Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Bransted-Lowry base, or neither reaction highlighted reactant Bronsted-Lowry Bronsted-Lowry acid base neither H, SO (aq) + NH3(09) - HSO (aq) + NH HSO (aq) + NH(aq) → H, SO. aq) + NH, (aq) H, SO (aq) + NH3(aq) - HSO (aq) + NH HSO (aq) + NH (0)...
#2 & 3
Identify the following species in water, as Bronsted Acids [A] or Bronsted Bases [B]: H_3O^+; H_2SO_4; OH^-; HCN; CH_3COOH; CH_3NH_2 WRITE NET Ionic Equations for the reactions of H_2PO_4^-, an amphiprotic ion, with aqueous solutions of HCl KOH Give the conjugate base for each of the following acids: HI HSO_4^- H_2CO_3 C_2H_5NH_3^+ Give the conjugate acid for each of the following bases: NH_3 O^2- H_2O PO_4^3- Identify the conjugate acid-base pairs in each of the following reactions:...
answer all parts clear and accurate
Indicate whether the following species are Arrhenius acids or bases and/or Bronsted-Lowry acids or bases: 1. Both Arrhenius and Bronsted acid 2. Bronsted base NH2 3. Bronsted acid HCIO 4. Arrhenius acid 5. Arrhenius base 6. Both Arrhenius and Bronsted base
Write equations for the reaction of each of the following Brønsted-Lowry acids and bases. Identify the conjugated acids and bases. a. Acid: H20; base: NH3 b. Acid: NH4+, base: OH- c. Acid: HSO4; base: H2O d. Acid: HCl; base: H2PO4 6.4
Identify the Bronsted acids and bases in the following equation (A-Bronsted acid, B = Bronsted base): CH3OH OH H2O CH30 a) A BBA b) BA BA c) A BA B d) BAA B
6. There are two major theories of acids and bases in aqueous solutions: Arrhenius and Bronsted. a) In your own words, briefly explain the main difference between the two theories of acids and bases b) Which theory do you think is the most useful in chemistry? Explain your choice. c) Which of the following is an Arrhenius acid? A) H2SO4: B) LiOH; C) NH2CH3; D) CH3CH3; E) More than one of these is an Arrhenius acid. d) Which of the...
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