. Magnesium hydroxide is used in many antacid medicines. This is due to all of the reasons below except a. since it is a base, it will neutralize acid b. it does not dissociate well, which means excess medicine is less harmful c. it can accept two protons per formula unit d. being a strong base makes it ideal for neutralizing HCl

__ AgNO3(aq) + __ K2CO3(aq) --> Full ionic:Net ionic: __ Ca(OH)2(aq) + __ H2SO4(aq) --> Full ionic:Net ionic:

15. a. Antacid is a substance which neutralizes stomach acidity (HClm) to relieve an upset stomach. The chemical used for such purpose normally is Mg(OH)2. Write the balanced equation for the neutralization reaction b. Sodium bicarbonate (baking soda) can also serve the same purpose but it is seldom used this way. Explain why it is so by writing out the bala nced equation for the reactions.

A. What is a diprotic acid? Give an example. B. Write an equation representing the reaction that would occur if only one mole of NaOH is reacted with one mole of H₂SO3. C. Write an equation representing the reaction that would occur if one mole of the product (the product containing S) from the reaction above is reacted with one mole of NaOH. D. Write a balanced equation for the complete neutralization of H2SO3 with NaOH. E. What is the relationship between the equation you wrote in "D" and the equations in "B" and "C"? F. Rewrite the equations above as net ionic equations. Does the same relationship still exist? G. H₂SO3 is a diprotic acid. Using the graph below, sketch an approximate curve of pH vs. vol. of NaOH added for what you expect to observe for the titration of H₂SO3 with the strong base NaOH. Discuss the shape of your curve with your instructor. 14 pH 405.90 29108A1 od 0- Deo volume of NaOH added odabos 94 Be ob son od adf tiba

2. Write reactions to show the dissociation into ions of the following substances when they dissolve in water: a) sodium phosphate b) ammonium hydroxide 3. Explain why water is such a good solvent for so many different solutes.

Part A - Solution 1 After being given a solution containing a set of unknown ions, you perform the following sequence of tests to determine the identity of the cations in solution: 1. A flame test produces no color 2. You take a small portion of the solution and add NaOH. A vapor is produced that turns red litmus blue. 3. You add HCI to solution, which results in the formation of a white precipitate. The supernatant is separated and used for the remainder of the tests. 4. The addition of buffered NH4*/NH3 to a portion of the supernatant from step 3 does not produce a precipitate. 5. The addition of ammonium oxalate to a portion of the superntant from step 3 does not produce a precipitate 6. The addition of a strong base to a portion of the supernatant from step 3 generates a precipitate. 7. The supernatant from step 6 is separated from the precipitate. The addition of HCI and K4Fe(CN)6 to the solution produces no reaction. Based on these tests, identify which of the following ions must…

I need help determining which compounds will ionize.

Which of these compounds are oxoacids (also known as oxyacids)? HF O hydrochloric acid chloric acid HCN H,PO, O Ba(OH), nitrous acid

The different between strong and weak acids and bases is that ... strong acids or bases are solutions of low concentration. only some molecules of a strong acid or base react with water. all of the molecules of a strong acid or base react with water. Selected strong acids or bases are solutions of high concentration. 2 UNANSWERED QUESTION 3/5 CONTINUE 4:16 / 13:48 1x X

Give the name of the following compounds, classify them as strong/weak/non-acid/base/electrolyte and write its reaction in water. 1. FeCrO4 2. Ba(OH)2 3. H2SO4 4. H3PO4 5. Formula for ammonium sulfate. Classify as well.