Questions :
1. The aqueous solutions of three compounds are shown in the diagrams. Identify each compound as a nonelectrolyte, a weak electrolyte, or a strong electrolyte .
a) nonelectrolyte solution .
b) strong electrolyte solution .
c) weak electrolyte solution .
2.Which of the following diagrams best represents the hydration of NaCl when dissolved in water? The Cl− ion is larger in size than the Na+ ion.
The diagram best represent the hydration is c
because NaCl Ions are separated and H positive Inos is attracted to Cl which are negative .
3.Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (a) H2O, (b) KCl, (c) HNO3, (d) HC2H3O2, (e) C12H22O11
a) nonelectrolyte
b) strong electrolyte
c) strong electrolyte
d) weak electrolyte
e) weak electrolyte
4.Predict and explain which of the following systems are electrically conducting: (a) solid NaCl, (b) molten NaCl, (c) an aqueous solution of NaCl
an aqueous and molten solutions of NaCl are electrically conducting because Ions in these solutions are separated which promote conducting electricity .
5.You are given a water-soluble compound X. Describe how you would determine whether it is an electrolyte or a nonelectrolyte. If it is an electrolyte, how would you determine whether it is strong or weak
The first step is to determine whether this compound is molecular or ionic , if it is ionic , it is , then , strong electrolyte . The second step comes when the compound is molecular to determine whether it is acidic , basic or neither , if it is basic , it is weak electrolyte . If it is
neither , it is nonelectrolyte . If it is acidic , is it listed in the strong electrolyte acidic molecular list , if so , it is , then , strong , if not , it is weak electrolyte
this diagram is helpful in solving such this questions
b) strong electrolyte solution .
c) weak electrolyte solution .
2.Which of the following diagrams best represents the hydration of NaCl when dissolved in water? The Cl− ion is larger in size than the Na+ ion.
The diagram best represent the hydration is c
because NaCl Ions are separated and H positive Inos is attracted to Cl which are negative .
3.Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (a) H2O, (b) KCl, (c) HNO3, (d) HC2H3O2, (e) C12H22O11
a) nonelectrolyte
b) strong electrolyte
c) strong electrolyte
d) weak electrolyte
e) weak electrolyte
4.Predict and explain which of the following systems are electrically conducting: (a) solid NaCl, (b) molten NaCl, (c) an aqueous solution of NaCl
an aqueous and molten solutions of NaCl are electrically conducting because Ions in these solutions are separated which promote conducting electricity .
5.You are given a water-soluble compound X. Describe how you would determine whether it is an electrolyte or a nonelectrolyte. If it is an electrolyte, how would you determine whether it is strong or weak
The first step is to determine whether this compound is molecular or ionic , if it is ionic , it is , then , strong electrolyte . The second step comes when the compound is molecular to determine whether it is acidic , basic or neither , if it is basic , it is weak electrolyte . If it is
neither , it is nonelectrolyte . If it is acidic , is it listed in the strong electrolyte acidic molecular list , if so , it is , then , strong , if not , it is weak electrolyte
this diagram is helpful in solving such this questions
The list of strong acidic molecular compounds :
- $$HCL$$
-$$HBr$$
-$$HI$$
-$$HNO_3$$
-$$HClO_3$$
-$$HClO_4$$
-$$H_2(SO)_4$$
-$$HSO_4$$
6.Write ionic and net ionic equations for the following reactions:
(a) AgNO3(aq) + Na2SO4(aq) →
(b) BaCl2(aq) + ZnSO4(aq) →
(c) (NH4)2CO3(aq) + CaCl2(aq) →
These two tables are helpful in solving this kind of questions :
a)
$$ AgNo_{3(aq)}+Na_2 (SO)_{4(aq)} \rightarrow 2Ag(So)_{4}+2Na(No_3)$$
Ionic equation :
$$2(Ag)^+ +2(No_3)^- +2(Na)^+ +(So_4)^{2-}\rightarrow \, Ag_2(So)_{4}+2(Na)^+ +2(NO_3)^-$$
net ionic equation :
$$2(Ag)^+ +(So_4)^{2-}\,\rightarrow Ag_2(So)_{4}$$
b)
$$ BaCl_{2(aq)}+Zn (SO)_{4(aq)} \rightarrow Ba(So)_{4}+ZnCl_2$$
Ionic equation :
$$(Ba)^{2+} +2(Cl)^{-} +(Zn)^{+2} +(So_4)^{2-}\rightarrow \, Ba(So)_{4}+(Zn)^{+2} +2(Cl)^-$$
Net Ionic equation :
$$(Ba)^{+2}+(So_4)^{-2}\,\rightarrow Ba(So)_{4}$$
c)
$$(NH_4)_2 Co_3+CaCo_3\rightarrow\, NH_4Cl+CaCo_3$$
Ionic Equation :
$$2(NH_4)^{+} +(Co_3)^{2-} +(Ca)^{2+} +2(Cl)^{-}\rightarrow \, Ca(Co)_{3}+2(NH_4)^{+} +2(Cl)^-$$
Net Ionic Equation :
$$(Ca)^{2+}+(Co_3)^{2-}\, \rightarrow \, CaCo_3$$
7.List the general properties of acids and bases.
- Acids has a sour taste whether Bases has a bitter taste .
- Acids and Bases are strong electrolytes
- Acids turn blue litmus red while Bases turn red litmus blue
8.Give Arrhenius's and Brønsted's definitions of an acid and a base. Why are Brønsted's definitions more useful in describing acid-base properties?
- Arrhenius Acid is a substance that produce a (H+) ions when it ionizes in water .
- Arrhenius Base is a substance that produce a (OH-) ions when it ionizes in water .
- Bronsted Acid is a proton donor .
- Bronsted Base is a proton acceptor .
Bronsted definitions are more convenient because Arrhenius's ones are restricted to the behavior of acids and bases in aqueous solutions .
9.Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.
- Monoprotic acid :
$$HCl$$
- Diprotic acid :
$$H_2So_4$$
- Triprotic acid :
$$H_3Po_4$$
10.What are the products of an acid-base neutralization reaction?
-Water and salts
11.What factors qualify a compound as a salt? Specify which of the following compounds are salts: CH4, NaF, NaOH, CaO, BaSO4, HNO3, NH3, KBr
- The factors are that salts are solids because they are a products of acid and base reaction and the salts must contain of a combination of an anion and a cation in which the cation isn't a (H+) and anion isn't
$$o^{2-}or (OH)^{-}$$
$$CH_4\, isn't a\, salt$$
$$NaF\, is\, a\, salt$$
$$NaOH, isn't\, a\, salt$$
$$CaO, isn't a\, salt$$
$$BaSo_4\, is\, a\, salt$$
$$HNO_3\, isn't a\, salt$$
$$NH_3\, isn't a\, salt$$
$$KBr\, is a\, salt$$
11.Identify the following as a weak or strong acid or base: (a) NH3, (b) H3PO4, (c) LiOH, (d) HCOOH (formic acid), (e) H2SO4, (f) HF, (g) Ba(OH)2
this figure below may be helpful.
$$-NH_3 \,is\,a\,weak\,base $$
$$-H_3Po_4\,is\,a\,weak\, acid $$
$$-LiOH \, is\,a\,strong\, base $$
$$-HCOOH \, is\, a\, weak\, acid $$
$$H_2So_4 is\, a\, strong\, acid$$
$$-HF \, is\, a\, weak\, acid$$
$$-Ba(OH)_2 \, is\, a\, Strong\, base $$
12.Identify each of the following species as a Brønsted acid, base, or both:
(a) $$HI$$
Both
(b) $$(C_2H_3O_2)^{-}$$
(c)
(d)
$$(Ba)^{+2}+(So_4)^{-2}\,\rightarrow Ba(So)_{4}$$
c)
$$(NH_4)_2 Co_3+CaCo_3\rightarrow\, NH_4Cl+CaCo_3$$
Ionic Equation :
$$2(NH_4)^{+} +(Co_3)^{2-} +(Ca)^{2+} +2(Cl)^{-}\rightarrow \, Ca(Co)_{3}+2(NH_4)^{+} +2(Cl)^-$$
Net Ionic Equation :
$$(Ca)^{2+}+(Co_3)^{2-}\, \rightarrow \, CaCo_3$$
7.List the general properties of acids and bases.
- Acids has a sour taste whether Bases has a bitter taste .
- Acids and Bases are strong electrolytes
- Acids turn blue litmus red while Bases turn red litmus blue
8.Give Arrhenius's and Brønsted's definitions of an acid and a base. Why are Brønsted's definitions more useful in describing acid-base properties?
- Arrhenius Acid is a substance that produce a (H+) ions when it ionizes in water .
- Arrhenius Base is a substance that produce a (OH-) ions when it ionizes in water .
- Bronsted Acid is a proton donor .
- Bronsted Base is a proton acceptor .
Bronsted definitions are more convenient because Arrhenius's ones are restricted to the behavior of acids and bases in aqueous solutions .
9.Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.
- Monoprotic acid :
$$HCl$$
- Diprotic acid :
$$H_2So_4$$
- Triprotic acid :
$$H_3Po_4$$
10.What are the products of an acid-base neutralization reaction?
-Water and salts
11.What factors qualify a compound as a salt? Specify which of the following compounds are salts: CH4, NaF, NaOH, CaO, BaSO4, HNO3, NH3, KBr
- The factors are that salts are solids because they are a products of acid and base reaction and the salts must contain of a combination of an anion and a cation in which the cation isn't a (H+) and anion isn't
$$o^{2-}or (OH)^{-}$$
$$CH_4\, isn't a\, salt$$
$$NaF\, is\, a\, salt$$
$$NaOH, isn't\, a\, salt$$
$$CaO, isn't a\, salt$$
$$BaSo_4\, is\, a\, salt$$
$$HNO_3\, isn't a\, salt$$
$$NH_3\, isn't a\, salt$$
$$KBr\, is a\, salt$$
11.Identify the following as a weak or strong acid or base: (a) NH3, (b) H3PO4, (c) LiOH, (d) HCOOH (formic acid), (e) H2SO4, (f) HF, (g) Ba(OH)2
this figure below may be helpful.
$$-NH_3 \,is\,a\,weak\,base $$
$$-H_3Po_4\,is\,a\,weak\, acid $$
$$-LiOH \, is\,a\,strong\, base $$
$$-HCOOH \, is\, a\, weak\, acid $$
$$H_2So_4 is\, a\, strong\, acid$$
$$-HF \, is\, a\, weak\, acid$$
$$-Ba(OH)_2 \, is\, a\, Strong\, base $$
12.Identify each of the following species as a Brønsted acid, base, or both:
(a) $$HI$$
Both
(b) $$(C_2H_3O_2)^{-}$$
(c)
(d)
ليست هناك تعليقات:
إرسال تعليق