Question

The ph range and buffer questions on photo 1 and questions 6,7, and 8 on the last photo please!

Lab 9 Lab Report Home Insert Page Layout Formulas Data Review View Q122 x fx B C D E F G 108 5. Determine buffer capacity and the pH range of your buffer 109 Produce a graph of pH vs. molarity of acid (and base) added to the buffer. You should end up with one Igraph with molarity of acid on the left of your graph (you will have to assign negative values to the acid imolarities) and molarity of base on the right of your graph (see the graph of buffer capacity on page 14). What is the pH range of your buffer? What is the buffer capacity for the addition of strong acid and for the 113 addition of strong base for your buffer? Table 5. Graph Data I do not insert any data in the gray cells) 110 111 112 pH range PH 0 Buffer capacity for the addition of strong acid = 5.82 Buffer capacity for the addition of strong base Molarity of Acid or Base added to Buffer, M 6.97 -4.76E-03 -9.09E-03 6.91 -1.30E-02 6.83 -1.67E-02 6.74 THCI) - Moles of HCI -2.00E-02 6.62 Total Volume (L) -2.31E-026.46 -2.59E-02 -2.86E-02 -3.10E-02 -3.33E-02 6.97 4.76E-03 7.02 9.09E-03 704 1.30E-02 7.12 1.67E-02 720 NaOH) = Moles of 2.00E-02 7.30 NaOH/Total Volume 2.31E-02 7.36 2.59E-027.42 2.86E-02 752 310E-02 7.72 3.33E-02 8.12 3.55E-02 3.75E-02 10.06 pH vs. molarity of acid (and base) Lab 9 Select destination and press ENTER or choose Paste

Answer 1

Buffer have a larger Gloacity for acid and base because a solution with more weak bose LAJ, has a higher luffer Capacity for addition of strong acid similarly a buffer will bore amount of strong base added is so lange it consumes. all the weak acid, through the rana HA + oH Á +Ho, Buffer solution is able to retain almost constant pH when small amount of acid I base is added Buffer Capacity can be also defined as quantity of strong acid or base that must be added to change I the pH of one liter of solution by pH unit. Buffers are solutions that resist changes in ph, upon addition of small amounts of acid or loase. The can do this because they contain an acidic component HA to neutralize of ions, and a basic component A to neutralize 4+ ions. when a small amount of acid is added to a butter solution, for example in an acetic aid buffer, the itional Hudrosen ions react with acetate ions to form acetic acid which is feebly iowized. In this case there is no raise in hydrogen ions concentration and of the solution is this ineffected. if we Similarly is we add a add a small small a amount of base for our lition, the additional hydroxide ion heill combine solution, the additional bus example u acetic quid to form heater to hich is hle. Hence the Hydronde concentration is C

unoffented which also makes the pot constant. when a small amount of an acud or base is added to a buffer solution, the PH is yo affected Conversely, when the same amount of aidſ base is added to an unbuffered system there will be a significant change in pH ..