A cation that is expected to act as a weak acid in water a. K+(aq) b....
A cation that is expected to act as a weak acid in water
a. K+(aq)
b. Ag+(aq)
c. Pb2+(aq)
d. Mg2+(aq)
Homework Answers
Weak acid won't ionize fully when dissolved in water. But backward reaction is more feasible. The cation with larger size will act as weak acid in water.
Pb2+ has larger size as it has 80 electrons.
Other cations K+ (18 electrons), Ag+ (46 electrons) , and Mg2+ (10 electrons) are having smaller size compared to Pb2+.
So, Pb2+ is expected to act as weak acid in water.
Answer is Option C.
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A cation that is expected to act as a weak acid in water
a. K+(aq)
b....
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urgent
I 4) For each of the following questions circle the correct answer. There is one and only one correct answer per problem.[5 points cach] a) A colligative property whose value depends directly on the mole fraction of solute particles boiling point freezing point vapor pressure osmotic pressure elevation depression lowering b) An example of a strong soluble base Pb(OH)4 Ba(OH)2 Cu(OH)2 AgOH c) A cation that is expected to act as a weak acid in water Mg2+(aq) Pb?" (aq)...
4) For each of the following questions circle the correct answer. There is one and only...
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For a generic weak acid HA, the ionization into H+ and A in water is not complete: HA (aq) =H+ (aq) + A (aq) a. Show that the acid dissociation constant of the acid, Ka, can be obtained from the degree of dissociation a using the following formula: a2 Ka 1-a b. The freezing-point depression of a 0.010 m acetic acid solution is 0.0193 K. From this data, what is the acid- dissociation constant K of acetic acid?
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1. (2 points) Silver ion, Ag+ (aq), oxidizes formaldehyde, CH2O(aq), to formic acid, HCOOH(aq). Write the balanced equation for this transformation in aqueous acidic solution. In your answer be sure to convert any H+(aq) that may be present to H30+ (aq) and to include states on all species. 2. (1point)At 25 °C the redox process Mn2+ (aq) + Mg(s) = Mn(s) + Mg2+ (aq) has the standard potential of Eºcell = +1.34 V. Calculate the equilibrium constant of this process...
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