Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of...
soluble blz dissociah. - A student mixed 5.00 mL of 0.0120 M Pb(NO), with 5.00 mL of 0.0300 M KI and observed a yellow precipitate. Show all calculations for each of the following questions. a. What is the molecular formula of the precipitate? 0.000mlm Co.0120) (-005) b. How many moles of Pbare present initially? (moles = M.V) c. How many moles of l' are present initially? 0.00016 moleso.03)00-05) . The concentration of l' at equilibrium is experimentally determined to be...
Thank you for the help! 2. A student mixed 5.00 mL of 0.0120 M Pb(NO,), with 4.00 mL of 0.0300 M KI and 1.00 mL of 0.20 M KNO, and observed the formation of a yellow precipitate. Show all calculations for each of the following questions. a. What is the molecular formula of the precipitate? b. How many moles of Pb2+ are present initially? (moles = M.V) c. How many moles of I- are present initially? d. The concentration of...
-8 3 Calculate the solubility of copper (10 lodate in 0.15 M copper (1) nitrate, K is 7.4x10M. "You should know that the Kan must refer to the copper lodate because all nitrate compounds are soluble and strong electrolytes Answer: Warm UP Question. What is the initial (before any reaction takes placel lead nitrate concentration when 8.0 mL of 0.111 M lead nitrate is added to 19 mL of 0.0070 M sodium chloride? Answer: K For the reaction: PbCl (s)...
1) A 110 mL solution of 0.340 M HCl(aq) is mixed with a solution of 330 mL of 0.150 M HNO3(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H+ are present in the final solution? 2) When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of Pblu, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the...
A solution composed of 5.00 mL of 0.0120 M Pb(NO3)2, 3.00 mL of 0.0300 M KI, and 2.00 mL of 0.20 M KNO, is determined Spectroscopically to have [1] -6.25 x 10" M. Show all steps of your calculations. Credit will not be given if work is not shown. a). How many moles of l' is present initially? (2 pt) S+3+2=100L OIL •BM= I 19x10 noles b). How many moles of I should precipitate from the solution? (2 pt)
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL of 0.150 M NiSO_4. (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?
A solution composed of 5.00 mL of 0.0120 M Pb(NO3)2, 3.00 mL of 0.0300 M KI, and 2.00 mL of 0.20 M KNO3 is determined spectroscopically to have [1'] = 6.25 x 10 Show all steps of your calculations. Credit will not be given if work is not shown. (2 pt) a). How many moles of l' is present initially? OIL OB S+3+2=10nL M = a. 1o-s b). How many moles of I should precipitate from the solution? " Xo...
5. If 75.0 mL of a 0.20 M solution of sodium nitrate (NaNO3) is mixed with 25.0 mL of 0.10 M barium nitrate (Ba(NO3)2), what is the molar concentration of nitrate in the resulting solution? A. 0.10 M D. 0.15 M B. 0.20 M E. 0.18 M C. 0.30 M
Experiment 26: The Solubility Product of Ba(IO3)2 : Processing the Data Experiment 26 Data and Calculations: The Solubility Product of Ba(IO3)2 The calculations here are similar to those in Experiment 23, and are outlined in the Experimental Procedure section. To use a spreadsheet, set up a table like the one below. Test Tube Number mL 0.0350 M KIO mL 0.0200 M Ba(NO3)2 1.00 2.00 3.00 4.00 5.00 5.00 5.00 5.00 5.00 5.00 12.00 12.00 12.00 12.00 12.00 0.382 0.396 0.804...
44.2 mL of aqueous 0.255 M Pb(NO3)2 is mixed with 31.6 mL of 0.415 M NaCl. The equation for the precipitate reaction is: Pb(NO3)2 (aq) + 2 NaCl (aq) --> PbCl2 (s) + 2 NaNO3 (aq) The concentration of NO3- ion in the reaction solution is _____ M.