a student used a 0.358 g sample of Alka-Seltzer and the mass of CO2 was found to be 0.102 g. Based on this result, answer the following questions:

Determine the mass of NaHCO3 that produced the CO2 in the experiment.

Determine the % mass of NaHCO3 in the sample.


Determine the mass of NaHCO3 in the tablet assuming the mass of the tablet is 3.50 g

How do I go about answering these questions?

yes

Well, let me break it down for you, my curious friend. To determine the mass of NaHCO3 that produced the CO2 in the experiment, you need to use some stoichiometry. The molar mass of CO2 is 44 g/mol, so you can calculate the moles of CO2 produced using its mass of 0.102 g. Then, use the balanced chemical equation of the reaction to find the mole ratio between NaHCO3 and CO2 to determine the moles of NaHCO3. Finally, convert the moles of NaHCO3 to grams using its molar mass of 84 g/mol.

Now, to determine the % mass of NaHCO3 in the sample, you'll need to divide the mass of NaHCO3 that you just calculated by the mass of the Alka-Seltzer sample (0.358 g) and multiply by 100 to get the percentage.

Regarding the mass of NaHCO3 in the tablet assuming the mass of the tablet is 3.50 g, you can simply multiply the % mass of NaHCO3 that you just calculated by the tablet mass to find the mass of NaHCO3 in the tablet.

Hope that answers your questions!

To answer these questions, you need to use stoichiometry and the balanced chemical equation for the reaction between NaHCO3 (sodium bicarbonate) and HCl (hydrochloric acid) in Alka-Seltzer tablets.

Let's start with the first question:

1. Determine the mass of NaHCO3 that produced the CO2 in the experiment:
First, you need to find the molar mass of CO2, which is 44.01 g/mol.
Then, use the stoichiometry of the balanced chemical equation:

2 NaHCO3 + 2 HCl -> 2 CO2 + 2 H2O + 2 NaCl

From the equation, we can see that 2 moles of NaHCO3 produce 2 moles of CO2.
Since you know the mass of CO2 produced (0.102 g), you can use the molar mass of CO2 to find the number of moles of CO2 produced.
0.102 g CO2 * (1 mol CO2/44.01 g CO2) = X moles CO2

Since the stoichiometric ratio between CO2 and NaHCO3 is 1:1, you can conclude that the moles of NaHCO3 used is the same as the moles of CO2 produced: X moles NaHCO3.

Finally, you need to convert the moles of NaHCO3 to grams using its molar mass (84.01 g/mol):
X moles NaHCO3 * (84.01 g NaHCO3/1 mol NaHCO3) = Mass of NaHCO3 in grams

Now, let's move to the second question:

2. Determine the % mass of NaHCO3 in the sample:
Based on the previous calculations, you know the mass of NaHCO3 that produced the CO2. Now, you need to find the percentage by mass of NaHCO3 in the total sample.

To do this, use the given mass of the Alka-Seltzer tablet (3.50 g). Subtract the mass of the CO2 produced (0.102 g) from it to find the mass of the remaining components (uncounted for yet).

3.50 g - 0.102 g CO2 = Mass of remaining components in grams

Then, divide the mass of NaHCO3 (from the previous calculation) by the total mass of the remaining components and multiply by 100 to get the percentage:

(Mass of NaHCO3 / Mass of remaining components) * 100 = % mass of NaHCO3 in the sample

I hope this explanation helps you. If you have any further questions, feel free to ask!

0.102 x (molar mass NaHCO3/molar mass CO2) = ? g NaHCO3.

% mass in sample = (mass NaHCO3/mass sample)*100 = ?