Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- In a titration, if 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point. What is the molarity of the vinegar solution? Hint: Vinegar contains acetic acid (HC2H3O2).arrow_forwardFor a buffer initially containing .08 mol of benzoic acid (HC7H5O2) and .12 mol of C7H5O2 in 1.0 L, what is the pH after .07 mol of OH is added to the buffer? .07 mol OH- .08 mol HC,H,O2 .12 mol C,H¿0; O 4.57 O 5.47 O 2.91 O 4.37 O 3.71arrow_forward#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)arrow_forward
- A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]arrow_forwardFor humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?arrow_forwardA 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? 227 g/mol 82.5 g/mol 371 g/mol 124 g/mol 186 g/molarrow_forward
- We have a titration for the titration of 50.0 mL of 0.425 M lactic acid, a monoprotic acid, (Ka = 1.38 x 10^-4) with 0.350 M NaOH. 1. Calculate the exact volume of the NaOH needed (to the correct numbers of sig figs) to reach the equivalence point. 2. Calculate the exact volume of NaOH needed (to the correct numbers of sig figs) to reach the mid point.arrow_forwardA certain indicator, HA, has a K value of 2.0 x 10. The protonated form of the indicator is blue and the ionized form is red. What is the pK, of the indicator? pK = What is the color of this indicator in solution with pH = 3? about us careers privacy policy terms of use contact us help 949 PM XI 风下 3/10/202 edts f12 inse ho 立arrow_forward7. The pH titration curve of a weak acid, HA, is shown me below. As the titration progresses, HA is converted into its conjugate base, A-. 12 10 8 (a) What is the volume of NaOH at the equivalence point? 2 25 30 35 15 20 volume of NaOH added (mL) 5 10 (b) At what volume (or volumes) is all of the acid present in the protonated (HA) form? (c) At what volume (or volumes) is all of the acid present in the conjugate base (A') form? (d) At what point along the titration will half the original amount of HA have been converted to A-?arrow_forward
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