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Concept explainers
(a)
Interpretation:
More acidic solution of
Concept Introduction:
An electrolyte refers to an ionic compound that on solvation in polar protic solvents ionizes to yield cationic and anionic species. The free movement of such ionic species results in the conduction of electricity.
Three subcategories exist for electrolyte namely strong electrolyte weak electrolyte and non-electrolyte. The strong electrolytes on dissolution exhibit
In contrast, the weak electrolytes are not
(b)
Interpretation:
More acidic solution of
Concept Introduction:
Refer to part (a).
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Chapter 15 Solutions
FOUND.OF COLLEGE CHEMISTRY
- Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?arrow_forwardClassify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3arrow_forwardWhat is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?arrow_forward
- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?arrow_forwardWrite two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.arrow_forwardYou purchase a bottle of water. On checking its pH, you find that it is not neutral, as you might have expected. Instead, it is slightly acidic. Why?arrow_forward
- A Liquid HF undergoes an autoionization reaction: 2HFH2F++F (a) Is KF an acid or a base in this solvent? (b) Perchloric acid, HCIO4, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction. (c) Ammonia is a strong base in this solvent. Write the chemical equation for the ionization reaction. (d) Write the net ionic equation for the neutralization of perchloric acid with ammonia in this solvent.arrow_forwardDifferentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?arrow_forwardStudents are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2arrow_forward
- The pH scale for acidity is defined by pH – log10 H*| where |H*| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of rain water is 5.5. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = Marrow_forwardConsider the aqueous solutions of two weak acids depicted in diagrams A and B. (a) What is the formula of the acid and conjugate base in each solution? (b) Which of the following Ka values corresponds to each acid: 3.4 × 10 −7 and 1.0 × 10 −2? (c) Which conjugate base is stronger?arrow_forwardAcidity of a solution is determined by the concentration H of hydrogen ions in the solution (measured in moles per liter of solution). Chemists use the negative of the logarithm of the concentration of hydrogen ions to define the pH scale, as shown in the following formula. pH = -log (H) Lower pH values indicate a more acidic solution. (a) Normal rain has a pH value of 5.6. Rain in the eastern United States often has a pH level of 3.8. How much more acidic is this than normal rain? (Round your answer to two decimal places.) 63.10 times as acidic as normal rain (b) If the pH of water in a lake falls below a value of 5, fish often fail to reproduce. How much more acidic is this than normal water with a pH of 5.6? (Round your answer to two decimal places.) * times as acidic as normal waterarrow_forward
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