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The following very strong acids are formed by the reactions indicated:
(a) Identify the Lewis acids and bases.
(b) To which atom is the H atom bonded in each acid?
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Chapter 16 Solutions
EBK GENERAL CHEMISTRY
- The formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why.arrow_forwardWhen carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)arrow_forward1. Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. NH₄Cl(aq) + KOH(aq) → 2. Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. NH₄Br(aq) + LiOH(aq) → 3. Balance the following chemical equation (if necessary): C₆H₆O(l) + O₂(g) → H₂O(g) + CO₂(g) 4. Balance the following chemical equation (if necessary): C₃H₆(g) + O₂(g) → CO₂(g) + H₂O(g)arrow_forward
- Reactions Which type of reaction is indicated by the following formula: 2A920 → 4Ag + O2 O Replacement O Decomposition O Synthesisarrow_forwardSuppose that a volume of 5.0 cm³ of acetic anhydride (density = 1.08 g·cm⁻³, molar mass = 102.087 g·mol⁻¹) is hydrolysed completely and the resulting solution is made up to 100.0 cm³ in a volumetric flask. Calculate the volume in cm³ of 0.496 mol·dm⁻³ sodium hydroxide required to titrate a 10.0 cm³ sample of this solution. [Round the answer to two decimal places. Do not type in the unit. Use a decimal point.] *arrow_forwardConsider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10arrow_forward
- If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.arrow_forwardComplete and balance the following acid-base neutralization reaction: 1 H2SO4 + 2 NAOHarrow_forwardZinc metal reacts with nitric acid, HNO, to produce a number of products, depending on how dilute the acid solution is. In a concentrated salution, zinc reduces nitrate ion to ammonium ion; zinc is oxidized to zinc ion, Zn Write the net ionic equation for this reaction.arrow_forward
- For each of the following pairs of substances • Classify each of the substances. • Compare their approximate pH levels. • Compare their ability to conduct electricity. • Compare their relative hydronium or hydroxide concentration. Comparison of 1.0 mol/L LIOH(aq) and 1.0 mol/L HOCI(aq) • LIOH(aq) is classified as a • HOCI(aq) is classified as a • HOCI(aq) has a + pH than LIOH(aq) has. . нос(ag) is a + electrical conductor than LIOH(aq) is. LIOH(aq) has a : [OH (aq)] than HOCI(aq) has. Comparison of 1.0 mol/L HCN(aq) and 1.0 mol/L KF(aq) • KF(aq) is classified as a • HCN(aq) is classified as a • HCN(aq) has a : pH than KF(aq) has. • HCN(aq) is a + electrical conductor than KF(ag) is. • HCN(aq) has a + [H30+(aq)] than KF(aq) has.arrow_forwardHypochlorous acid (HCIO) is a weak acid. The conjugate base of this acid is the hypochlorite ion (CIO). Wrtie a balanced equation showing the reaction of HClO with water. Include phase symbols. balanced equation: C₁0(aq) +H₂0(1) → HO Write a balanced equation showing the reaction of CIO with water. Include phase symbols. balanced equation:arrow_forwardA 0.150 mol · L 1 solution of a weak base (B) has a pH of 11.28. Part A Based on the pH, determine [OH ] at equilibrium for this weak base solution. Express your answer to two significant figures. [OH-] = 1.9-10_3 mol · L-1 Submit Previous Answers Completed Part B At equilibrium, [OH ] = 1.9x10-3 mol - L-1, which is also the concentration of the conjugate acid BH+. Based on this, determine Kh for the weak base B. Express your answer using two significant figures. ? K = Submit Request Answerarrow_forward
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