Fundamentals Of Analytical Chemistry
9th Edition
ISBN: 9781285640686
Author: Skoog
Publisher: Cengage
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- Solution 1 Solution 2 Solution 3 Solution 4 Solution 5 Concentration iron(III) nitrate 0.00200 0.00200 0.00200 0.00200 0.00200 [Fe(NO3)3] (M) Concentration potassium thiocyanate 0.00200 0.00200 0.00200 0.00200 0.00200 [KSCN] (M) Volume Fe(NO3)3 (mL) 5.00 5.00 5.00 5.00 5.00 Volume KSCN (mL) 5.00 4.00 3.00 2.00 1.00 Volume DI water (mL) 0.00 1.00 2.00 3.00 4.00 Initial concentration [Fe3+] (M) 0.00100 0.00100 0.00100 0.00100 0.00100 Initial concentration [SCN] (M) 0.00100 0.000800 0.000600 0.000400 0.000200 Absorbance 0.269 0.192 0.154 0.104 0.052 Equilibrium [FeSCN2+] (M) 0.000198 0.000141 0.000113 0.0000765 0.000038 Equilibrium constant Kc Average Kcarrow_forward(d) A sample contains a mixture of ammonium carbonate (NH4)2CO3, sodium carbonate Na2CO3, and sodium chloride NaCl. Thermogravimetric analysis indicates that a 0.0965-g portion of this sample loses 0.0574 g over a temperature range of 50-75 oC and then loses another 0.0124 g at 800 oC.(i) What causes the weight loss at 50-75 oC? (ii) What species will remain after being heated to 800 oC? (iii) What is the composition of the original sample? Given: Atomic masses: H = 1.008; C = 12.011; N = 14.007; Na = 22.99; O = 15.999;Cl = 35.45.arrow_forwardHow many of the following reactions will Kc = Kp? • H2(g) + I2(g) = 2 HI(g) • N204(g) = 2NO2(g) • S03(g) + NO(g) = SO2(g) + NO2(g) • 2 HgO(s) = Hg(1) + O2(g) • CH4(g) + H2O(g) = CO(g) + 3 H2(g) • (s) + 02(g) = CO2(g) 1 4 2 3arrow_forward
- I need help solving this problem (see attached)arrow_forwardThe Ksp for SrF2 is 2.45 x 10-9. Use this information to calculate the solubility of Strontium Fluoride in water (find the [Sr2+] and [F-] at equilibrium). SrF2 (s) Sr2+ (aq) + 2F- (aq) I C Earrow_forwardWrite the expression for Keq for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous.(a) N2(g) + 3 H2(g) 2 NH3(g) Keq = PNH32 / (PN2 PH23) Keq = (PN2) (3 PH2) / 2 PNH3 Keq = PN2 PH23 / PNH32 Keq = 2 PNH3 / ((PN2) (3 PH2)) homogeneous or heterogeneous. (b) 4 HCl(g) + O2(g) 2 H2O(l) + 2 Cl2(g) Keq = PHCl4 PO2 / PCl22 Keq = 2 PCl2 / (4 PHCl PO2) Keq = 4 PHCl PO2 / 2 PCl2 Keq = PCl22 / (PHCl4 PO2)arrow_forward
- Write the expression for Keq for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous.(a) N2(g) + 3 H2(g) 2 NH3(g) Keq = PNH32 / (PN2 PH23) Keq = (PN2) (3 PH2) / 2 PNH3 Keq = PN2 PH23 / PNH32 Keq = 2 PNH3 / ((PN2) (3 PH2)) The reaction is (b) 4 HCl(g) + O2(g) 2 H2O(l) + 2 Cl2(g) Keq = PHCl4 PO2 / PCl22 Keq = 2 PCl2 / (4 PHCl PO2) Keq = 4 PHCl PO2 / 2 PCl2 Keq = PCl22 / (PHCl4 PO2) The reaction is (c) H2(g) + I2(g) 2 HI(g) Keq = 2 PHI / (PH2 PI2) Keq = PH2 PI2 / 2 PHI Keq = PH2 PI2 / PHI2 Keq = PHI2 / (PH2 PI2) The reaction isarrow_forwardThe Ksp of CAF2 is 1.5 x 10-10, If CaF2 (s) is dissolved in pure water, what is the solubility in grams per liter (g/L)? О 2.6 х 10:2 O 6.8 x 10-4 О 3.3 х 10:2 O 4.1 x 10-2 О 3.3 х 10-4arrow_forward20) What is the value for Kc if [CO] = 0.025, [H2]= 0.013 and [CH3OH] = 0.0028 for the following reaction? %3D CH3OH(g) =CO(g) +2 H2(g) A) 0.12 В) 1.5 х 10-3 C) 9.1 x 10-7 D) 6.6 × 102 E) 8.6arrow_forward
- (Q46) Given that the molar solubility of copper (1) chloride (99.00 g/mol) at 25°C is 4.15 x 10-4 mol/L, it follows that at equilibrium: O 41.1 mg of CuCl will exist in one liter of solution as a precipitate 41.1 mg of CuCl will be dissolved in one liter of solution O 41.1 mg of precipitate and 41.1 mg of dissolved ions will be present in one liter of solution O Increasing the temperature would have no effect on solubiility O Diluting the solution would cause precipitation to beginarrow_forwardGiven that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.arrow_forwardA group of wealthy chemistry 1A students had a little too much disposableincome and decided to create the most expensive they could think of. Using various spectroscopictechniques the salt was determined to be rhodium (III) Bromide (RhBr3). When this salt was shaken withpure water at 25°C, the solubility was found to be 0.026 mg/mL. Calculate the Ksp of RhBr3arrow_forward
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