Precipitation of Šilver lon HCI(aq) Test/reagent used: Chemical(s) responsible for precipitation: Choose.. Confirmatory Test NH.OH(aq) and HNO:(ac Test/reagent used: Chemical(s) responsible for a positive test: Choose...

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Are you completing this experiment online? Yes Part A Data. Standardization of a Sodium Hydroxide Solution Data Table 1. Measurements for standardization of NaOH Data Table 1. Measurements for standardization of NaOH Trial 1 Trial 2 Trial 3 [1] Tared mass of KHC8H404 (g) 0.335 0.308 0.383 [2] Burette reading of NaOH, initial (mL) 3.75 3.91 4.15 [3] Burette reading of NaOH, final (mL) 19.83 18.14 21.36 Part B Data. Molar Concentration of an Acid Solution Enter the number corresponding to the type of acid you have 1. НА 1 2. H2А 3. НзА

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Indicate the concentration of each ion present in the solution formed by mixing the following. (a) 22 mL of 0.100 M HCl and 10.0 mL of 0.220 M HCl H+ = ________ M ; Cl- = _________M (b) 15.0 mL of 0.300 M Na2SO4 and 29.2 mL of 0.100 M NaCl Na+= _________M;  (SO4)2- = ____________M; Cl- = _________M (c) 3.50 g of KCl in 60.0 mL of 0.404 M CaCl2 solution (assume that the volumes are additive) K+= _____________M ; Ca+= ______________M ; Cl- = ___________M

Write an analysis scheme using HCl (write in formulas of precipitated) for cations Ag, Pb, and Zn.    Then evaluate your results. How well did the scheme work? What problems did you encounter?

During a lab experiment performed at STP conditions, you prepare HCl by reacting 100. ml of Cl2 gas with an excess of H2 gas. How many ml of a solution of Ba(OH)2 0.230M do you need to neutralize all the HCl produced? ** Please provide a clear and detailed explanation of the process so that I can follow along. Thank you so much for your help!

If 17.1 mL of 0 M NaOH are used, how many moles are in this sample? Suppose 0.371 grams of a solid monoprotic acid are titrated with 16.45 mL of 0.117 M NaOH.  What is the molar mass of the solid acid?

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

Solid potassium chromate is slowly added to 125 mL of a 0.440 M barium nitrite solution until the concentration of chromate ion is 0.0127 M. The percent of barium ion remaining in solution is   %?