CHEM105 Study Guide - Final Guide: Weak Base, Conjugate Acid, Rice Chart

17. Which of the following statements aboat fitration curvei is false? a In titration curves for weak acid weak base, pH chinges near the equivalcoce point too small for color changes to be used b. The equivalence point will be basic when titrating a weak acid with a strong bale c. A titration curve for titrating a strong acid strong base will always have an point at pH 0. Gdy The end point of titration is the point where chemically equivalent amounts of acid and 18, e have reacted bow pH changes near the equivalence point. A shows which of followi statements about buffers is the a The pled buffer Molu will no drastically wben small amounts of strong b acid or strong base change A always con of a weak acid or weak base, and a soluble ionic salt of the weak acid or weak ba c. Most body contain natural systems d. A buffer solution buffer e. The pH can with either H ious. of a buffer solution witll change drastically when diluted with asmall anwouet of 19. Which one of the following combinations is net a buffer solution? b. NH, NH CIO. c, HNO, NaNo, id. HNO, LiNO's e, HF RhFe 20. The nonionized form of an acid indicator is yellow, and its anion is blue. The K of this indicator 10 What will be the approximate pH range over which this indicator changes color? b, 5-7 9-11 e, 8-10 21. A solution contains 0,20 M Au o 20 M cu and o.20 M Ag ions when LiCI is added to the solution what is the order in which the chloride salts will begin to precipitate? K roa" 1.8 x 10 K 10-1) 107 a. CuCl AgCl AuCl 22. Which of the following solubility product expressions is incorrect?

Adding a strong Acid to a Buffer Part A Learning Goal : A beaker with 145 mL of an acetic acid buffer with a pH of 5,000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.60 mL of a 0.320 M HC1 solution to the beakerHow much will the pH change? The pK, of acetic acid is 4.740. To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH Express your answer numerically to two decimal places. Use a minus (-) sign if the pH has decreased. Hints A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH, COOH, and its conjugate base, the acetate ion CH3 COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (eg., sodium acetate NaCH COO). IVO Aze s o o o ? ApH -- 0.363 Submit My Answers Give Up Incorrect, Try Again; 5 attempts remaining Buffers work because the conjugate acid-base pair work together to neutralize the addition of H' or OH ions. Thus, for example, if H ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of Hwith the conjugate base: Provide Feedback Continue H+ + CH, COO CH, COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid OH + CH3 COOHCHCOO + H2O This buffer system is described by the Henderson-Hasselbalch equation [conjugate base] pH = pK. log [conjugate acid)