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A 0.2349g sample of an unknown acid requires 33.66mL of 0.1086M NaOH for neutralization to a phenolphthalein end point. There are 0.42mL of 0.1049M HCl used for back-titration.
a. How many moles of OH- are used? How many moles of H+ from HCl?
b. How many moles of H+ are there in the solid acid?
c. What is the molar mass of the unknown acid?
When 210.0mL of 0.350M K2CrO4(aq) are added to 210.0mL of 1.10×10^?2M AgNO3(aq), what percentage of the Ag^+ is left unprecipitated
a compound was analyzed and was found to contain the following percentages of the elements by mass barium 89.56 oxygen
Explain how these products are produced by showing the mecahnism involved. (draw).
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what kind of inter-molecular interactions would likely dominate? explain your reasoning
Complete the table for aqueous solutions of caffeine C8H10O2N4. a. given: mole fraction solven:0.900 find molality, mass percent solvent, Ppm solute b. given: Ppm solute:1269 find molality, mass percent solvent,
Propose a synthetic method to carry out the transformation shown, using any additional organic or inorganic reagents. 5 methyl 1 hexyne ----> 7 methyl 3 octene
NH3 is a weak base (Kb = 1.8 × 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.041 M in NH4Cl
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What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl.
The Ka of acetic acid is 1.85 x 10-5. What would be the pH of a buffer prepared by mixing 50.0 mL of 1.0 M potassium acetate with 50.0 mL of 1.0 M acetic acid?
A 120.0mL buffer solution is 0.105M in NH3 and 0.135M in NH4Br. What amount of HCl could this buffer neutralize before it fell below 9.0 pH
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