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Basic Chemistry
- Consider the equilibration of a weak base B (K, = 7.63 × 10¬³) between water (phase 1) and benzene (phase 2). %3D Which expression represents D, the distribution ratio? B Which expression represents KD, the distribution represents the unprotonated form of the base and BH+ constant? B represents the unprotonated form of the base represents the protonated form of the base. O [B]2 [B]] and BH† represents the protonated form of the base. [B]2 [B]] + [BH*]] [BH*]2 [BH*]2 [BH+]1 [B]] + [BH*]1 [BH*]2 [BH*]] [B]2 [B]] + [BH*]] [BH*]2 [B]2 [B]] + [BH*]] [B]] Calculate D at pH 8.41 if Kp = 49.0. Will D be larger or smaller at pH 6.00 than at pH 8.41? %3D smallerarrow_forward1) A 10mL solution of 3M HCI is diluted to 50mL. What is the concentration of the 50mL solution? 2)In Beer’s law (A=abc), what corresponds to y,m,x and b in the equation of a line (y-mx + b)? Note that b is not the same in the two equations. 3)You have two solutions containing the same compound having the same pink color. The concentration of the first solution is 2.0M, while the concentration of the other solution is 2.5M. Absorbance of each solution was measured with the same spectrophotometer at the same wavelength. a) Which solution has the more intense pink color? b) Which solution has the higher absorbance?arrow_forwardA certain indicator, HA, has a ?a value of 7.9×10^−7. The protonated form of the indicator is yellow and the ionized form is red. What is the p?a of the indicator? p?a= A generic salt, AB2, has a molar mass of 287g/mol and a solubility of 2.80 g/L at 25 °C. AB2(s)↽−−⇀A2+(aq)+2B−(aq) What is the ?sp of this salt at 25 °C? ?sp=arrow_forward
- Acetic acid is a weak acid. Its formula is CH3COOH. Only the last H is an acid proton. Vinegar is usually 5 % (v/v) acetic acid. If 25.00 mL of vinegar is titrated by a standardized 0.9315 M NaOH solution, it takes 22.38 mL to reach the endpoint. Calculate the molarity of acetic acid in the 5 % (v/v) vinegar.arrow_forward1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1) Initial Buret Reading (mL) Final Buret Reading (mL) Volume Base Added (mL) 2 => Na Mg Rb Sr 2.92 M Cs Ba 0.55 M 1.21 M Be 0.97 M 1.76 M Ca Sc 3.11 M Ra La 91 AM Hf Ac Trial 1 0.3 14.2 TI Zr Nb Mo Tc [81 $4 Cr Mn Fe Re Os Rf Db Sg Bh Hs Periodic Table of the Elements T Trial 2 14.2 A Basic D 30.0 Symbol 10 77 78 224, Co Ni Cu Zn Ga B 14 Neble Gas Trial 3 30.0 43.9 Ru Rh Pd Ag Cd In Sn Sb Te M с N Expe 201 VIA Sm Nd Pm Eu Gd Dy Ho "Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 15 VIA M He Ge As Se Br Kr Xe Pt Au Hg Ds Rg Cn Uut FI Uup Lv Uus Uuo Ne "Er Tm Ybarrow_forwardA 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K = 4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 5.00 mL of NaOH are added to the analyte? Question 4 A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K, -4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 10.00 mL of NaOH are added to the analyte? Assume Ku = 1.0 x 10-14 Using the titration curve below for the titration of 10.00 mL of the analyte NH3 with HCl(aq) (titrant) to estimate pKa for NH3 Titration of 10.00 mL Ammonia (ag) with Hydrochloric Acid (ag) 12.0 11.0 10.0 9.0 8.0 7.0 5.0 4.0 3.0 2.0 1.0 0.0 0.0 2.0 4.0 10.0 12.0 140 16.0 180 20.0 6.0 Volume of HCI Added (mL) 8.0arrow_forward
- What are the concentrations of H+ and OH− in asolution of 0.02 M NaOH?arrow_forwardThis question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…arrow_forwardYou are titrating a 1.033 g sample of white vinegar solution (5.0% acetic acid) with a 1.00 M NaOH titrant. At the endpoint of titration, 0.89 mL of NaOH was used. What is the mass % of acetic acid based on your experimental results? CH3COOH = 60.052 g/molarrow_forward
- If we spill a Strong Base in the laboratory, there is a squeeze bottle ofWeak acid available to completely neutralize the spill. a) What volume (in liters) of 0.40 M CH 3 COOH is required to completelyneutralize 20.0 mLs of 0.80 M KOH? Do not round off your answer. b) What is the pH at the Equivalence Point? ka CH 3 COOH =1.8 x 10 -5arrow_forwardThis is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid? The reaction is: H3PO4 (aq) + 3 NaOH (aq) → Na3PO4 (aq) + 3 H2O (l)arrow_forwardThe equivalent weight for an acid is the molar mass divided by the number of moles of H + (for a base it is the molar mass divided by the number of moles of OH-) that enter a particular reaction. For the reaction given, what is the equivalent weight for hydrochloric acid? 3HCI+Al(OH)3-3H2O+AICI3arrow_forward
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