The expression for Kb ( i.e base dissociation constant ) tells about the ability of the base to gain H+ ion from the aqueous medium generally . When any species accepts H+ ion from the medium then this base forms its conjugate acid.
As water can acts as both acid and base so , here it is acting as an acid to release its H+ ion .
Hence the Kb expression should be like
B) HSO3- + H2O
OH- + H2SO3
Here Lithium bisulfite ions dissociate completely being an strong electrolyte so , its bisulfite ion reacts with water to form sulphurous acid ( H2SO3 ) and hydroxyl ions ( i.e OH- ) .
Kb = [ OH- ] [ H2SO3 ] / [ HSO3- ]
As here water is not included in this expression because it is present in excess and its concentration is not changing with time .
Write the equation that represents the Kh of LiHSO3. O А HSO3 + H20=H30+ + 50%-...
For which of the following reactions will the reactants be favored at equilibrium? NH3(aq) + H30+ (aq) = NH4+ (aq) + H20(1) CO32- (aq) + H30+ (aq) = HCO3(aq) + H2O(1) CH3COOH(aq) + OH(aq) = CH3COO" (aq) + H2O(1) HSO3- (aq) + H3O+ (aq) =H2SO3(aq) + H2O(1) CIOA" (aq) + H3PO4(aq) = HCIO4(aq) + H2PO4" (aq)
Write a balanced base equation for F"(aq) F (aq) + H20(1) =H30+ (aq) + HF (aq) F"(aq) + H20(1) = H20"(aq) + F(aq) F (aq) + H2O(0) = OH"(aq) + HF(aq) F"(aq) + H20(1)=H*(aq) + HOF(aq) Impossible to determine QUESTION 2 Write a balanced base equation for CH3CH2NH2(aq) CH3CH2NH2(aq) + H2O(1) = H30+ (aq) + CH3CH2NH" (aq) CH3CH2NH2(aq) + H2O(1) = OH(aq) + CH3CH2NH3(aq) CH3CH2NH2(aq) + H2O(1) = H20" (aq) + CH3CH2NH2+(aq) CH3CH2NH2(aq) + H2O(1) = NH4+(aq) + CH3CH2OH(aq) Impossible...
14 Which one of the equation ons helow represents that happens when Niis dissolved in water? | Hà N | | | | | | | | NIHOONIS NON + OH- NHÀ | | | | |-- VỊ | | | | | | * | | | 15 What is the change in the hange in the oxidation number of chromium in the following K Cr:07 - Cr(SO:)3 a increase by three units h increase by four units decrease...
7. a) Identify the conjugate acid-base pairs in the following reaction: NH3(aq) + H O(l) + NHa*(aq) + OH (aq) b) The conjugate acid of HCO3 ? c) The conjugate base of H2PO4? d) Which of the following is not a conjugate acid-base pair? A) NH4+/NH3; B) H30*70H; C) H2SO3/HSO3; D) C2H3027HC2H302; E) All of the above are conjugate acid-base pairs.
complete the following
reactions. A) i) 1. MgBr O 1. LICH2CH3 2. H20 2. H30+ j) b) 1. MgBr
OCH3 1.
PLS PLS PLSSS help me with these.
a) i) 1. MgBr O 1. LICH2CH3 2. H20 2. H30+ j) b) 1. MgBr OCH3 1. CH3Li 2. H20 2. H30* c) k) OH 1. CH3 MgBr 2. H20 OH 1. CH3Li 2. H20 d) 1) MgBr 1. CH20 2. H307 1. (CH3)3CMgBr 2. H20 H 3 1. MgBr 2. H30*...
complete the following reactions.
a) i) 1. MgBr O 1. LICH2CH3 2. H20 2. H30+ j) b) 1. MgBr OCH3 1. CH3Li 2. H20 2. H30* c) k) OH 1. CH3 MgBr 2. H20 OH 1. CH3Li 2. H20 d) 1) MgBr 1. CH20 2. H307 1. (CH3)3CMgBr 2. H20 H 3 1. MgBr 2. H30* 1. Mg Br 2. CO2 3. H20 OCH3 n) f) 1. CH3CH2MgBr 2. H20 1. Li CI 2. CH3CH2OH OH o) g) Br 1....
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...
A) H20 c) нсоз- E) H2CO3 DOH. 22) Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? A) In acids, [OH-] is greater than [H3O* B) In bases, [OH-]- [H3o*]. C) In neutral solutions, [H3O"] = [H20]. D) In bases, [OH-] is greater than [H3o*]. E) In bases, [OH-] is less than [H30*]. 23) Which of the following is a buffer system? A) NaCl(aq) and NaNO3(aq) C) H2CO3(aq) and KHCO3 (aq) E) H20(0) and HCl(aq)...
15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is best explained by the equation: A) NO3-(aq) + H2O(1) + HNO3(aq) + OH(aq) B) Fe3+(aq) + 6 H2O(1) Fe(OH)3(aq) + 3 H30+(aq) C) [Fe(OH2)6]3+(aq) + H20(1) 3 H3O+(aq) + [Fe(OH2)5(OH)]2+(aq) D) H3O+(aq) + OH-(aq) + 2 H2O(1) E) HNO3(aq) + H2O() H30+(aq) + NO3-(aq)