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23 Nov 2019

Which of the 5 common active ingredients (Mg(OH)2, Al(OH)3, NaHCO3,CaCO3, MgCO3) is the most effective, by mass, at neutralizingexcess stomach acid? Show calculations to prove your answer.

(*I think it's Al(OH)3 because that would neutralize 3 moles ofHCl. I'm not sure how to prove it though.*)

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Bunny Greenfelder
Bunny GreenfelderLv2
6 May 2019

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Related questions

Please workout on paper.

1. On the web do a search for MSDS sodium sulfate, barium cholride, sodium chloride, and barium sulfate. Tell me their colors and solubilities.

2. How would an increase in the concentration of the reactants affect the moles of reactant?

3. Explain the role of limiting and excess reagents in any chmical experiment.

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1. Calculate the maxiumum volume in mL of 0.15 M HCl that each of the following antiacid formulations would be expected to neutralize. Assume complete neutralization.

a. A table containing 250 mg Al(OH)3 and 150 mg Mg(OH)2

b. A tablet containing 850 mg of CaCo3

2. A student is given an antiacid tablet that weighed 5.6832 g. The tablet was crushed and 4.3628 g of the antiacid was added to 200 mL of simulated stomach acid. This was allowed to react and then filtered. It was found that 250-mL of this partially neutralized stomach acid required 8.50 mL of a NaOH solution to titrate it to a methyl red endpoint. It took 21.54-mL of this NaOH solution to neutralize 25.00-mL of the original stomach acid.

a. How much of the "stomach acid" had been neutralized in the 25.00-mL sample which was titrated? (Show work.)

b. How much stomach acid was neutralized by the 4.3628 g sample used? (Show work.)

c. How much stomach acid would have been neutralized by the original 5.6832 g tablet? (Show work.)

1.A tablespoon (tbsp) is how many teaspoons (tsp)?

1/2/3/4

2.A metal pan made of cast iron will take longer to heat than an aluminum pan because iron has a (lower.higher) thermal conductivity than alumium

Cast iron has a (lower/higher) pecific heatthan aluminum, meaning it will take less energy to heat up iron than aluminum to the same temperature, assuming the same mass*.

3.Which materials are not good for cooking acidic foods such as tomatoes because the metal will react with the acid?

Pooly seasoned cast iron or non-anodized alumium / stainless steel / glass / copper

4.When measuring out solid ingredients, you fill the measuring cup with the item and then use a knife to cut across it for an even top/level. For brown sugar only (which is compressible), you should (pack it/ spoon sugar into the cup / scoop nomally

when filling the measuring cup or else there will be (less / more) sugar than what is called for.

5.When measuring one cup of a fluffy substance (such as flour) how should you measure it, assuming you are using a measuring cup rather than a balance.

(A balance would be the best way as it measures mass rather than volume which is often more accurate!)

1.Scoop it into the measuring cup then level i

2. Scoop it using the measuring cup then level it

3. Pack it so it's more dense

4. Use tablespoons to measure it out

6. When measuring ingredients, mass (grams, pounds, ounces) measures ( amount of substance there is / the amount of space a substances takes up)

whereas volume (cups, tbsp, quarts, gallons) measures ( amount of substance there is / the amount of space a substances takes up)

Balance the following Chemical Equations:

____Fe(s) + ____H2O(g) ® ____Fe3O4(s) + ____H2(g)

____C2H6(g) + ____O2(g) ® ____CO2(g) + ____H2O(g)

(C) ___ KClO3 (s) ® ___ KCl (s) + ___ O2 (g)

___ C6H14 (l) + ___ O2 (g) ® ___ CO2 (g) + ___ H2O (g)

___ C3H8O3 (l) + ___ O2 (g) ® ___ CO2 (g) + ___ H2O (l)

___ NaN3 (s) ® ___ Na (s) + ___ N2 (g)

__ C3H5N3O9 ® __ CO2 + ___ N2 + ___ H2O + ___ O2

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H2O(g) + C(s) ⟶ CO(g) +H2(g)

(B) 2KClO3(s) ⟶ 2KCl(s) +3O2(g)

(C) Al(OH)3(aq) +3HCl(aq) ⟶ AlCl3(aq) + 3H2O(l)

(D) Pb(NO3)2(aq) + H2SO4(aq) ⟶ PbSO4(s) + 2HNO3(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H3PO4

(B) Al(OH)3

(C) SeO2

6. Complete and balance the following acid-base equations:

(A) A solution of HClO4 is added to a solution of LiOH.

(B) Aqueous H2SO4 reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)2(aq) + HC2H3O2(aq) ⟶

(B) H3PO4(aq) + CaCl2(aq) ⟶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. Ans: 1.67 g Mg

9. H2 is produced by the reaction of 118.5 mL of a 0.8775-M solution of H3PO4 according to the following equation: 2Cr + 2H3PO4 ⟶ 3H2 + 2CrPO4. How many grams of H2 are produced? Ans: .315 g H2

10. Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.

2NaN3(s) ⟶ 2Na(s) + 3N2(g)

What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN3

11. Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO2 produced by combustion of 1.00 x 104 grams of CO2?

CO2(g) + 2NH3(g) ⟶ CO(NH2)2(s) + H2O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H2SO4(l) ⟶ HCl(g) + NaHSO4(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO3(s)⟶CaO(s) + CO2(s)

Ans: 92.0 %

14. Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C12H22O11 + H2O +3O2 ⟶2C6H8O 7+ 4H2O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of O2 react according to P4+5O2 ⟶ P4O10?

(B) Calculate the percent yield if 10.0 g of P4O10 is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N2 ⟶ Li3N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point?

AgNO3(aq) + NaCl(aq) ⟶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO3)2 solution.

2Cl−(aq) + Hg(NO3)2(aq) ⟶ 2NO3−(aq) + HgCl2(s)

What is the Cl− concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO3)2(aq) to reach the end point?

Ans: 0.009636 M

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