(a)
Interpretation: Assign oxidation numbers to all of the elements in HSO4-
Concept Introduction: The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(b)
Interpretation: Assign oxidation numbers to all of the elements in H3PO3
Concept Introduction: The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(c)
Interpretation: Assign oxidation numbers to all of the elements in Cr2O72-
Concept Introduction: The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
(d)
Interpretation: Assign oxidation numbers to all of the elements in Na2CO3
Concept Introduction: The rules for assigning oxidation number to elements are:
- For an element in its free state it is assigned an oxidation number of zero.
- Monatomic ions have oxidation number that is equal to charge of the monatomic ion.
- Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.
- In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.
- For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.
If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.
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Basic Chemistry
- Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?arrow_forwardBalance each of the following oxidationreduction reactions by using the oxidation states method. a. C2H6(g) + O2(g) CO2(g) + H2O(g) b. Mg(s) + HCl(aq) Mg2+(aq) + Cl(aq) + H2(g) c. Co3+ (aq) + Ni(s) Co2+(aq) + Ni2+(aq) d. Zn(s) + H2SO4(aq) ZnSO4(aq) + H2(g)arrow_forwardBalance each of the following oxidationreduction reactions by nsing the oxidation states method. a. Cl2(g) + Al(s) Al3+(aq) + Cl(aq) b. O2(g) + H2O(l) + Ph(s) Ph(OH)2(s) c. H+(aq) + MnO4(aq) + Fe2+(aq) Mn2+(aq) + Fe3+(aq) + H2O(l)arrow_forward
- Balance each of the following oxidationreduction reactions by using the oxidation states method. a.C2H4(g) + O2(g) CO3(g) + H2O(g) b. Mg(s) + HCl(aq) Mg2+(aq) + Cl(aq) + H2(g) c.Co3+(aq) + Ni(s) Co2+(aq) + Ni2+(aq) d.Zn(s) + H2SO4(aq) ZnSo4(aq) + H2(g)arrow_forwardClassify each of the following reactions as a precipitation, acid-base, or gas forming reaction. Show states for the products (s, , g aq), and then balance the completed equation. Write the net ionic equation. (a) MnCl2(aq) + Na2S(aq) MnS + NaCl (b) K2CO3(aq) + ZnCl2(aq) ZnCO3 + Kaarrow_forwardBromine is obtained from sea water by the following redox reaction: Cl2(g) + 2 NaBr(aq) 2 NaCl(aq) + Br2() (a) What has been oxidized? What has been reduced? (b) Identify the oxidizing and reducing agents.arrow_forward
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