Data Table1 Concentration od HCl(M) Data Table 2. Experimental Results. I observ

Question

Data Table1

Concentration od HCl(M)

      

Data Table 2. Experimental Results.

I observed a solution go from being clear to a hot pink color in a matter of several droplets of NaOH into an antacid, HCl, and phenolphthalein solution.

If an antacid tablet weighed 1.6 grams, how many moles of gastric acid (HCl) would it neutralize? Use the results obtained in Data Tables 1 and 2 to explain and quantify your answer.

If you performed this experiment with a titrant of 0.5M NaOH, would you expect your results in Data Table 2 to change or stay the same? Explain your answer.

I'm really unsure how to figure these out. I am not even sure if Table 2 was answered correctly. If you see a mistake in table 2 could you tell me how to fix it?

Trial1 Trial2 Average

Concentration od HCl(M)

1 M 1M 1M Volume HCL (mL) 5 mL 5mL 5mL Concentration of NaOH (M) 1 M 1M 1M Initail NaOH Volume (mL) 9 mL 8 mL XXXXXX Final NaOH Volume (mL) 7.2 mL 6.6 mL XXXXXX Total Volume of NaOH Used (mL) 1.8 mL 1.4 mL 1.6 mL Mass of Crushed Antacid (g) 0.5 0.5 0.5

Explanation / Answer

Table 2 :

HCl available for neutralization = 1 M x 5 ml = 5 mmol

Average volume of NaOH used = 1.6 ml

Moles of NaOH used to neutralize excess HCl = 1 M x 1.6 ml = 1.6 mmol

HCl neutralized by antacid = 5 - 1.6 = 3.4 mmol

HCl neutralized per gram of antacid = 3.4 mmol x 36.5 g/mol/1000 x 0.5 g = 0.25

Now If we had 1.6 g antacid.

Moles of HCl it would neutralize = 1.6 g x 3.4 mmol/0.5 g = 10.88 mmol

Again If we performed the experiment with 0.5 M NaOH instead of 1 M. The volume of NaOH used would be double. However the moles of HCl available for reaction with antacid and NaOH would remain the same. Thus, the data in Table 2 would remain the same.

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