Question -1
F- accept H+ and form HF and OH-
so answer is third option.
Question -2
Amines are the derivative of ammonia and they are lewis base so they accept H+ and form their cation and release OH-
Answer is second option.
Please hit like button.
Write a balanced base equation for F"(aq) F (aq) + H20(1) =H30+ (aq) + HF (aq)...
estion 10 of 65 > Consider the reaction. HF(aq) + KOH(aq) — KF(aq) + H20(1) What is the net ionic equation for the chemical reaction? HF(aq) + K+(aq) + OH(aq) — K+(aq) + F (aq) + H2O(1) O HF(aq) + K+(aq) + OH-(aq) — K+(aq) + F (aq) + H+(1) + OH-(1) O HF(aq) + OH-(aq) —> F-(aq) + H2O(1) HF(aq) + K+(aq) F (aq) + H+(1) HF(aq) + K+(aq) K+(aq) + H2O(1) - 11 of 65 > Calculate either...
Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) = NH4+ (aq) + OH- (aq) Check all that apply. H2O/NH3 NH4+/NH3 H2O/OH NH4+/OH- Submit Request Answer Part B OH(aq) + HF(aq) = H20(1)+F- (aq) Check all that apply. H2O/F- H20/OH HF/F- HF/OH
Write a balanced equation for the dissociation of the Brønsted-Lowry acid HSO, in water OHSO4 (aq) + H2O(1) = H2SO4(aq) + OH"(aq) O HSO4 (aq) + H20(1) - 503(8) + OH(aq) + H,00 OHSO4 (aq) + H2O(l) = 5032 (aq) + OH"(aq) O HSO (aq) + H2011) - S02 (aq) + H2O(1) OHSO4 (aq) + H2O(1) = SO42(aq) + H30*(aq)
Identify the conjugate base in the equation below. HCIO(aq) + H20(1) clo- (aq) +H30+ (aq) Select one: a. Clot- b. HCIO c. H20 d. H301+ What species is the acid in the equation below? S2-(aq) + NH4+ (aq) + HS-(aq) + NH3(aq) Select one: a. S2 b. NH21+ c. HST- d. NH3 What species is the base in the equation below? S2(aq) + NH4+ (aq) + HS - (aq) + NH3(aq) Select one: a. S2 b. NH41+ C. HS1 d....
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).
"equation above" is CH3CH2NH2+H20 ==> CH3CH2NH3^+ +OH^- Write the K. equation for ethylamine, CH CH NH), using your balanced reaction above. For weak bases, an ICE table must be used to determine the equilibrium concentration of H.O. Follow Example 14.13 to see how this is done. Create an ICE table for a 0.150 M solution of ethylamine. CHỊCH,NH, (aq) + H2O (1) thg Calculate the pow and the pH of a 0.150 M solution of ethylamine. The K, value is...
QUESTION 13 Which equation shows a weak acid in water? LIOH(s) ---> Li+ (aq) + OH" (aq) HF (aq) + H20(1) ++ H30+ (aq) + F"(aq) Hl(aq) DD@ H+ (aq) + (aq) HCl(aq) + H2O(aq) ---> C1-(aq) + H30+(aq)
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator) HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator) HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
5. In the following reactions, identify the conjugate acid-base pairs. H2SO4 (aq) + H2O(1) → H30+ (aq) + HS0ǐ (aq) 1st pair: CH-NH2(aq) + H20(f) CH3NH扎aq) + OH-(aq) 1st pair: HF(aq) + NH3(aq) 근 NH (aq) + F-(aq) 1t pair: a. 2nd pair: 2nd pair: 2nd pair: