How can we answer question 4 and 5 ? 4) When Al, Mg and Ca act as the active ingredient in antacid medications they exist as hydroxide salts. Investigate how these salts would work to neutralize the acids in our stomach and then write the eqwation for this acid-base neutralization reaction explaining this. 5. An antacid tablet was dissolved in 26.00 mL of 0.650 M HCI. The excess acid was back-titrated with exactly 11.44 mL of 1.05 M Na0H. The average weight of a tablet is 0.834 g. The tablet came from a bottle of 200 tablets that cost $5.99. a) Calculate the moles of HCI neutralized by the tablet. b) Calculate the mass effectiveness of the antacid. c) Calculate the cost effectiveness of the antacid.

Question 25 of 30 Submit You prepare a standard NAOH solution for the laboratory, using potassium hydrogen phthalate (KHC§H,0a, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/ mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC6H,O6, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.74 mL of the NaOH to titrate (react exactly with) | % 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00

The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl.  How would you classify the species being titrated in this titration? diprotic weak base monoprotic weak base triprotic weak acid triprotic weak base diprotic weak acid monoprotic weak acid

Question 7