The following data were obtained when a Ca2+ ISE was immersed in standard solutions whose ionic strength was constant at 2.0 M. Ca2+ (M) E (mv) 3.27x 10-5 -75.1 3.27x10-4 -47.0 3.27x10-3 -18.8 3.27x 10-2 +9.30 3.27x10-1 +37.4 (a) Prepare a calibration curve and find the least-squares slope and intercept and their standard deviations. slope 428.13 4951.08 407 intercept Sy (b) The Nernst Equation tells us the equation values based on theory, but the data we collect in the lab often doesn't exactly agree with theory. Calculate the value of the slope correction value in the equation below. Response of Ca2+ electrode: E = constant + 0.05916log(ACa2+)(outside) (c) For a measured potential, the calibration curve gives us log [Ca²+ ]. We can compute [Ca²+] = 10log [Ca 2+ ]. Using rules for propagation of uncertainty in the Summary uncertainty for a sample that gave a reading of -23.8 ± 0.5 mV in four replicate measurements. Rules for Propagation Uncertainty table, calculate [Ca2+- M

The following data were obtained when a Ca2+ ISE was immersed in standard solutions whose ionic strength was constant at 2.0 M. Ca2+ (M) E (mv) 3.27x 10-5 -75.1 3.27x10-4 -47.0 3.27x10-3 -18.8 3.27x 10-2 +9.30 3.27x10-1 +37.4 (a) Prepare a calibration curve and find the least-squares slope and intercept and their standard deviations. slope 428.13 4951.08 407 intercept Sy (b) The Nernst Equation tells us the equation values based on theory, but the data we collect in the lab often doesn't exactly agree with theory. Calculate the value of the slope correction value in the equation below. Response of Ca2+ electrode: E = constant + 0.05916log(ACa2+)(outside) (c) For a measured potential, the calibration curve gives us log [Ca²+ ]. We can compute [Ca²+] = 10log [Ca 2+ ]. Using rules for propagation of uncertainty in the Summary uncertainty for a sample that gave a reading of -23.8 ± 0.5 mV in four replicate measurements. Rules for Propagation Uncertainty table, calculate [Ca2+- M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

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7-11. Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.541 3 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCI, and heating to dissolve the solid and expel CO2: CACO3 (s) +2H* → Ca²* +CO,T +H2O Calcium carbonate FM 100.086 The excess acid required 39.96 mL of 0.100 4 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
3- The aqueous solubility of CaSO, at 25 °C as 0.5 g CaSO4/100 mL. What is the Ksp of CaSO4 CaSO(s) = Ca²*(aq) + SO,²¯(aq) Ksp = ?
Use the expression of the activity coefficient to calculate the coefficient of activity of cobalt in the equilibrium solubility of Co (OH) 2 (Ksp = 1.3 x 10-15) in the presence of a solution containing 0.0333M NaCl. ions α: αCo 2+ = 0.45nm, αOH- = 0.30nm, -log γx = 0.51 zx2 √µ 1 + 3.3 αx√µ Select one:to. 0.51b. 0.91c. 0.75d. 0.83
Calculate the solubility of BaSO4 solid in 0.0167 M Ba(NO3)2 solution, taking into activity ( Keq=1.1x10-10 for BaSO4 , activity of Ba++=0.46 and activity of SO4-2=0.44)
For the dissociation of iodic acid, HIO3(aq) + H20(1) H3O*(aq) + I03 (aq) If, at equilibrium, [HIO3(aq)] = 0.16 mol L-1, [H30*(aq)] = 0.29 mol L-1, and [103 (aq)] = 0.21 mol L1, calculate Ko. (Give 2 significant figures in your answer.) Answer:
Calibration of a glass electrode gave a reading of 134.9 mV with a 0.05 m potassium hydrogen phthalate buffer standard ( pH = 4.015), and a reading of -69.1 mV with a 0.08 m HEPES, 0.08 m NaHEPES, 0.08 m NaCl buffer standard (pH = 7.454), both measured at 30 °C. What is the observed slope (mV/pH unit) of the calibration curve? slope observed slope theoretical What is the theoretical slope at 30 °C? pH -58.1 5.29 Incorrect What is the pH of an unknown that gives a reading of 41.4 mV with this electrode at 30 °C? Incorrect Incorrect mV/pH mV/pH
A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!
Calculate the ionic strength of a saturated solution of La(IO3)3 with 0.010 M La(NO3)3. Kp = 1.0 x 10-I| 9.05 x 10- 6.05 x 10-2 4.68 x 10-3 1.21 x 10- 9.36 x 10-3
A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+ ions. Use this value to calculate the Ksp of AgCl
Given the following reactions and their equilibrium constants,calculate the value for the overall formation constant forAg(NH3)2+. In addition, write the equilibrium expression forthe formation of Ag(NH3)2+.½Ag+(aq) + ½Cl–(aq) ⇋ ½AgCl(s) K1 = 7.45 x 104Ag(NH3)2+(aq) + Cl–⇋ AgCl(s) + 2NH3(aq) K2 = 323Ag+(aq) + 2NH3(aq) ⇋ Ag(NH3)2+(aq) Kf = ?