Homework Answers
24. The net Ionic equation for the reaction of strong aid and base is
H3O+ + OH- --> 2H2O
Option b is the right answer
25. H2SO4 is the strong bronsted Lowry acid as it can dissociates completely into H+ and SO4-2.
26.NaBr is the salt formed by strong acid and strong base. Hence this gives neutral pH around 7 when dissolved in water. Option D is the right answer.
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QUESTION 24 Which is a net ionic equation for the neutralization of a strong acid with...
Which one of the following salts, when dissolved in water, produces the solution with the highest...
Which one of the following salts, when dissolved in water, produces the solution with the highest pH? HINT: Remember that BASES have high pH. Mgo CH3NH31 LICIO4 O NaHSO4 Which of the following are weak diprotic acids? hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4 carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3COOH O carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3 formic acid - HCOOH, acetic acid...
Part A Which is a net ionic equation for the neutralization reaction of a strong acid...
Part A Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base? Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base? HCl(aq) + NH3(aq) ↔ NH4Cl(aq) H3O+(aq) + NH3(aq) ↔ NH4+(aq) + H2O(l) HCl(aq) + NaOH(aq) ↔ H2O(l) + NaCl(aq) H3O+(aq) + OH-(aq) ↔ 2 H2O(l)
Write a net ionic equation to show that nitric acid, HNO3, behaves as an acid in...
Write a net ionic equation to show that nitric acid, HNO3, behaves as an acid in water. + H2o(l) Submit Answer Retry Entire Group 5 more group attempts remaining Use the References to access important values if needed for this question. Acid Conjugate base H,S HS Acid Strength Increases Base Strength Increases HCiO CIO (1) Write a net ionic equation for the reaction between H2S and CIO that shows H2S behavin g as a Bronsted-Lowry acid BL acid BL base...
Write a net ionic equation to show that methylamine, CH3NH2, behaves as a Bronsted-Lowry base in...
Write a net ionic equation to show that methylamine, CH3NH2, behaves as a Bronsted-Lowry base in water. BL base BL acid BL base BL acid + H2O (aq) Submit Answer Retry Entire (g) B more group attempts remaining
Write a net ionic equation to show that hydrocyanic acid behaves as a Brønsted-Lowry acid in...
Write a net ionic equation to show that hydrocyanic acid behaves as a Brønsted-Lowry acid in water. BL BL acid BL base BL acid base Write a net ionic equation to show that ethylamine, C2H5NH2, behaves as a Bronsted-Lowry base in water. BL BL base BL acid BL base acid + H20 Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. + CIO = HSO3 + HCIO H2SO3(aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry...
QUESTION 13 Which equation shows a strong acid in water? LiOH(s) ---> Li+ (aq) + OH"...
QUESTION 13 Which equation shows a strong acid in water? LiOH(s) ---> Li+ (aq) + OH" (aq) HF (aq) + H20(1) 6+ H30+(aq) + F"(aq) HF(aq) ++ H+ (aq) + F"(aq) HCl(aq) + H2O(aq) ---> C-(aq) + H30+(aq).
please help Question Completion Status: QUESTION 11 Which one is correct answer for Kb? CN (aq)...
please help
Question Completion Status: QUESTION 11 Which one is correct answer for Kb? CN (aq) + H20 (1) + HCN (aq) + OH- (aq) ОА OB.F (aq) + H20 (1) + HF(aq) + OH-(aq) OC Zn(OH)6 (aq) + H2O(l) — [Zn(OH)5(OH2)]+ e- 2+ HCN(aq) + F(aq) + CN (aq) + HF(aq) E. Both A and B is for Kb Click Save and Submit to save and submit. Click Save All Answers to save all answers. QUESTION 12 of the...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
The correct answer is the 3rd one. NO3- has more charges and thus is more unstable...
The
correct answer is the 3rd one.
NO3- has more charges and thus is more unstable than water, so
wouldn't it be more likely for it to accept H+, making it a
stronger Bronsted-Lowry base compared to H20? (aka, Why is water
better at accepting H+ than NO3-?)
F- should be the strongest Bronsted-lowry base because HF is a
weak acid and thus its CB is more unstable (that's why it doens't
really want to donate its H+) -> an...
Question Completion Status: QUESTION 16 Which one of the following pairs cannot be mixed together to...
Question Completion Status: QUESTION 16 Which one of the following pairs cannot be mixed together to form a buffer solution? NH3, NH4Cl NaC2H302, C2H302H (C2H302- = acetate) B. O NaF, HF O D.NaCl, HCI H3PO4, KH P04 OE QUESTION 17 colmats the facoltinn hat er da Hand Min Click Save and sharque and submit. Click Save to say all are Remaining Time: 1 hour, 21 minutes, 41 seconds. Question Completion Status: Let's suppose that the pH of a solution of...
Which one of the following salts, when dissolved in water, produces the solution with the highest pH? HINT: Remember that BASES have high pH. Mgo CH3NH31 LICIO4 O NaHSO4 Which of the following are weak diprotic acids? hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4 carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3COOH O carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3 formic acid - HCOOH, acetic acid...
Write a net ionic equation to show that nitric acid, HNO3, behaves as an acid in water. + H2o(l) Submit Answer Retry Entire Group 5 more group attempts remaining Use the References to access important values if needed for this question. Acid Conjugate base H,S HS Acid Strength Increases Base Strength Increases HCiO CIO (1) Write a net ionic equation for the reaction between H2S and CIO that shows H2S behavin g as a Bronsted-Lowry acid BL acid BL base...
Write a net ionic equation to show that methylamine, CH3NH2, behaves as a Bronsted-Lowry base in water. BL base BL acid BL base BL acid + H2O (aq) Submit Answer Retry Entire (g) B more group attempts remaining
Write a net ionic equation to show that hydrocyanic acid behaves as a Brønsted-Lowry acid in water. BL BL acid BL base BL acid base Write a net ionic equation to show that ethylamine, C2H5NH2, behaves as a Bronsted-Lowry base in water. BL BL base BL acid BL base acid + H20 Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. + CIO = HSO3 + HCIO H2SO3(aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry...
QUESTION 13 Which equation shows a strong acid in water? LiOH(s) ---> Li+ (aq) + OH" (aq) HF (aq) + H20(1) 6+ H30+(aq) + F"(aq) HF(aq) ++ H+ (aq) + F"(aq) HCl(aq) + H2O(aq) ---> C-(aq) + H30+(aq).
please help
Question Completion Status: QUESTION 11 Which one is correct answer for Kb? CN (aq) + H20 (1) + HCN (aq) + OH- (aq) ОА OB.F (aq) + H20 (1) + HF(aq) + OH-(aq) OC Zn(OH)6 (aq) + H2O(l) — [Zn(OH)5(OH2)]+ e- 2+ HCN(aq) + F(aq) + CN (aq) + HF(aq) E. Both A and B is for Kb Click Save and Submit to save and submit. Click Save All Answers to save all answers. QUESTION 12 of the...
The
correct answer is the 3rd one.
NO3- has more charges and thus is more unstable than water, so
wouldn't it be more likely for it to accept H+, making it a
stronger Bronsted-Lowry base compared to H20? (aka, Why is water
better at accepting H+ than NO3-?)
F- should be the strongest Bronsted-lowry base because HF is a
weak acid and thus its CB is more unstable (that's why it doens't
really want to donate its H+) -> an...
Question Completion Status: QUESTION 16 Which one of the following pairs cannot be mixed together to form a buffer solution? NH3, NH4Cl NaC2H302, C2H302H (C2H302- = acetate) B. O NaF, HF O D.NaCl, HCI H3PO4, KH P04 OE QUESTION 17 colmats the facoltinn hat er da Hand Min Click Save and sharque and submit. Click Save to say all are Remaining Time: 1 hour, 21 minutes, 41 seconds. Question Completion Status: Let's suppose that the pH of a solution of...
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