Interpretation: It is given that, common nitrogen compounds having oxidation states ranging from
Concept introduction: Atoms lose or gain electrons to acquire stable state. Oxidation state is a number that is assigned to each element in a compound. This number describes the ability to loss or gain electrons.
To determine: The rationalization of range of oxidation state of common nitrogen compounds; some special properties for each substance given in Table
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Chemistry: An Atoms First Approach
- The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; ClO- is reduced to Cl-. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S2O3; I2 is reduced to I-. The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S4O6. In this analysis, potassium iodide was added in excess to 5.00 mL of bleach (d=1.00g/cm3) . If 25.00 mL of 0.0700 M Na2S2O3 was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of NaClO in the bleach?arrow_forwardThe Ka value for chlorous acid (HCIO2) is 1.1 × 102, while the Ka for nitrous acid (HNO2) is 4.6 x 10-4. Calculate the equilibrium constant of the reaction of HCIO2 with NO2. Predict whether the reaction equilibrium favors reactants or products. Consider the equilibrium system described by the chemical reaction below.. HCIO2(aq) + H2O(1) = H;0*(aq) + CIO, (aq) 1 Set up an expression for the Ka of chlorous acid (HCIO2) in water. Do not combine or simplify terms. Ка 1.1 x 102 5 RESET 1.1 x 102 4.6 x 10-4 [H;O*] [CIO2] [HCIO2] [H2O] [H3O*)? [CIO2 ? [HCIO2]? [H2O]? 2[H3O*] 2[CIO,] 2[HCIO2] 2[H20] 2.2 x 10-2 9.2 x 10-4 1.2 x 10-4 2.1 x 10-7arrow_forwardList the following compounds in order of increasing acid strength: HBrO, HBrO2, HClO2arrow_forward
- Explain, using Le Châtelier’s principle, why the equilibrium constant for the formation of NO from N2 and O2 increases with increasing temperature?arrow_forwardFor HClO2, Ka= 1.2 × 10-2. What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and [HClO2] = 0.203 M?arrow_forwardCalculate the pKa of hypochlorous acid. The pH of a 0.015 M solution of hypochlorous acid has a pH of 4.64.arrow_forward
- Which of the following statements is false regarding hydrogen peroxide? Reaction of H2O2 with Fe2+ ions will generate OH radicals. H2O2 can reduce Ce4+ under any conditions. H2O2 can oxidize Ce3+ in acidic solutions. Decomposition of H2O2 to form O2(g) and H2O(l) releases energy.arrow_forwardWhat is the pH of a 0.237 solution of sodium hypobromite (NaOBr)? The Ka of hypobromous acid is 2.24 x 10-9.arrow_forwardWrite and balance the Chemical Equation:HC2H3O2 + CaCO3→ calcium acetate + H2O + carbon dioxidearrow_forward
- Place the following in order of increasing acid strength. HlO < H1O 2 < HlO 3 < HlO 4; HIO 4arrow_forwardWrite the balanced equation for the neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. neutralization reaction:arrow_forwardwhy is nitrogen 2 not more basic?arrow_forward
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