a) HCl and HF both are acids.
Hence there is no reaction between these two compounds.
But HCl is stronger acid than HF. Hence in presence of HCl, there is no dissociation of HF due to common ion effect.
HCl ------> H+ + Cl-
There exists an equilibrium between proton and fluoride ion in case of weak acid where as strong acid dissociates completely.
HF <--------> H+ + F-
b)
NaOH and NH3 are both are bases. Hence there is no reaction between them.
NaOH is a stronger base than Ammonia. Hence NaOH dissociates completely where as in Ammonia, there exists an equilibrium between ammonium ion and OH- ions.
c) Neutralization Reaction between HCl(acid) and NaOH (base) forms a salt (NaCl) and water.
HCl + NaOH -------> NaCl + H2O
d) Neutralization Reaction between Ammonia (weak base) and acetic acid (weak acid) can be written as
CH3COOH + NH3 (aq) ------- > CH3COONH4 + H2O
f)
Ammonium chloride is a salt and Ammonia is a base. Hence no acid base reaction.
But in the presence of Ammonium chloride, dissociation of ammonia decreases due to common ion effect.
5. Write an acid-base equation for the following pairs of compounds: a. HF and HCI b....
2. Classify the following as strong or weak acids/bases. Write balances equations that describe the dissociation of the compounds in water. a. HF b. NH3 c. NaOH d. C6H5NH2 e. HNO2 f. CH3COOH g. HCI h. H2CO3 3. Please the species in each of the following groups in order of increasing acid strength. a. HIO3, HCIO3, HBrO3 b. HF, HI, HCI c. HOCI, HOI, HOF e. H2O, H2S, H2Se f. HBO, HBrO2, HBrO4, HBrO3
find the pH of these compounds. use 5% approximation where nescessary. say each compund has molarity of 0.10M HCl H2S04 strong acicd! the first proton comes off completely and [HSO4] NaOH NH3 NH4CI CH3COOH Ka 1.8 x 10-5 CH3COONa Kb(CH3COO) 5.6 x 1010 . .solve the quadratic equation. strong base Kb 1.8 x 10-5 Ka(NH4) 5.6 x 1010 HCl H2S04 strong acicd! the first proton comes off completely and [HSO4] NaOH NH3 NH4CI CH3COOH Ka 1.8 x 10-5 CH3COONa Kb(CH3COO)...
need help asap please Use the acid/base dissociation constants on the back page of this worksheet Which of the following mixtures result in the formation of a buffer when 1.0 L of each of the following solutions are mixed? 1. a. 1.0 M NaOH and 2.0 M CH3COOH b. 1.0 M NaOH and 2.0 M NH3 c. 1.0 M HCl and 2.0 M HCN d. 1.0 M HNOs and 2.0 M NaF e. 1.0 M NaOH and 1.0 M H2CO3...
All of the following are acid-base conjugate pairs EXCEPT A. HPO42-, PO43- B. H3O+, OH- C. CH3COOH, CH3COO- D. NH4+, NH3 E. H2O, H3O+
4. Write balanced molecular and ionic equations for following reactions: a. CaCOs(s) and HCI(aq) b. Well 5CINi(NO32 NaOH and HCl(aq) c. HCI(aq) NH3(aq) d. CH3COOH(aq)+ NaOH(aq)
Which of the following is the acid-base combination that cannot use phenolphthalein as an acid-base indicator? Select one: a. HBr and NH3 b. HF and KOH C. CH2COOH and NaOH d. HCI and LiOH
6. Complete the following acid base reactions, indicate the conjugate acid-base pairs, and state whether the reaction has a large or small equilibrium constant. a. CH3COOH(aq) + NH3(aq) = b. H2CO3 (aq) + NO3- (aq) = H2CO3 (aq) + H20 (0) = d. HCO3- (aq) + H2O (1) = (HCO3- is amphoteric!) e. NH3 (aq) + H20 (1) =
1. Which one of the following compounds is a Bronsted-Lowry base? a) CH3CO2 b) NH3 c) H2SO4 d) HCl e) CH3 2. Which compound do you expect to have the lowest pKa? a) HCl b) NH3 c) CH3CH2OH d) CH4 e) H2SO4 3. Which compound do you expect to have the lowest pKa? a) HCl b) NH3 c) CH3CH2OH d) CH4 e) H2SO4 4) What is the strongest base? a) CH3COOH b) CH3COO- c) CH3CH2OH d) CH3CH2O-
1. Write a chemical equation for the following: a) HNO and KOH b) HCl and NH3 c) HF and HC d) CHCOOH and NH e) CHCOOH and NaOH f) HSO and SO,
Acid Base ⇄ Conjugate Acid Conjugate Base (A) CH3COOH H2O ⇄ (B) NH3 H2O ⇄ (C) ⇄ HF OH− (D) H2O → I− (E) C5H5NH+ H2O ⇄ [H+] [OH−] pH pOH Acid, Base or Neutral (A) 1.0x10−3 M (B) 4.5x10‒8 M (C) 9.45 (D) 1.33