Formät Tools Add-ons Normal text I U A E - E - E E X Arial 11 GD 2 3 6. solution Post Lab questions: 1. What is the normal pH range of blood? Is blood acidic, basic, or neutral? Write the formulas of the buffer components that are present in blood to maintain its pH. Solution is acidic, basic, or neutral? [H3O+ ] [OH-] PH 4.4x10^-8 4.56 x 10-2 7.35 basic 3.5 x 10-3 2.8x10^-7 7.45 basic 1.58x10^-8 6.3x10^-7 7.8 basic 1.0x10^-7 1.0x10^-7 7.0 neutral 3.0x10^-4 3.33 x 10-11 3.52 acidic 3. Calculate the molarity of the HCI solution if 0.074 mol of HCI is dissolved in water to make 2000 mL of solution. Also calculate the pH of this solution. Hint: In case of strong acids the [H30 + ] is the same as the molarity of the acid. Vol 2000ml=2.0001 Moles of HCI dissolved=0.074 mol. mol/vol Hence concentration of H3O+(H+)(H3O+)= Mol 0.037 Hence ph=-log (H3O+)=-log(0.037)+1-43 4. State one advantage and one disadvantage of the red cabbage indicator and of the pH meter used in this experiment +

For the following, mix equal volumes of one solution from Group I with one solution from Group II to achieve the indicated pH. Calculate the pH of each solution. Group I: 0.20 M NH4Cl, 0.20 M HCl, 0.20 M C6H5NH3Cl, 0.20 M (C2H5)3NHCl Group II: 0.20 M KOI, 0.20 M NaCN, 0.20 M KOCl, 0.20 M NaNO2 a. the solution with the lowest pH b. the solution with the highest pH c. the solution with the pH closest to 7.00

Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?

The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.

A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein

. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.

Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?

Calculate the pH of each of the following solutions. a. 0.10 M CH3NH3Cl b. 0.050 M NaCN

What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?

What is meant by the presence of a common ion? How does the presence of a common ion affect an equilibrium such as HNO2(aq) H+(aq) + NO2-(aq) What is an acidbase solution called that contains a common ion?