Q.18 - An Introduction to General, Organic, and Biological Chemistry

Question

One tums tablet contains 500mg of calcium carbonate.

a. What is the formula of calcium carbonate?

b. What is the molar mass of calcium carbonate?

c. How many moles of calcium carbonate are in one roll of Tums that contains 12 tablets?

d. If a person takes two Tums tablets, how many grams of calcium is obtained?

e. If the daily recommended quantity of $C{a}^{2+}$ to maintain bone strength in older women is 1500mg how many Tums tablets are needed each day to supply the needed calcium?

Step-by-Step Solution

Answer

Part a. $CaC{O}_3$

Part b.$100.088 g$

Part c. $0.06 mole$ 

Part d. $0.4 g$

Part e. $3$ tablets

Step 1: Given Information (Part a)

Calcium carbonate is a dietary enhancement utilized when how much calcium taken in the eating routine isn't sufficient. Calcium is required by the body for sound bones, muscles, sensory system, and heart. Calcium carbonate additionally is utilized as an antacid to ease indigestion, acid heartburn, and irritated stomach.

Step 2: Explanation Part (a)

The formula of calcium carbonate is $CaC{O}_3$.

Step 3: Explanation Part (b)

Molar mass is calculated as,

Ca = $40.078 \mathrm{g}$

C = $12.01 g$

O = $16g$

Molar mass of $CaC{O}_3$ is,

$$\begin{gathered} =(1\times 12.01 \mathrm{g} \mathrm{C})+(1\times 40.078 \mathrm{g} \mathrm{Ca})+(3\times 16 \mathrm{g} \mathrm{O}) \\ =100.088 g \end{gathered}$$

Step 4: Explanation Part (c)

The moles of calcium carbonate are in one roll of Tums that contains $12$ tablets is,

The amount of calcium carbonate in $12$ tablets is,

$12\times 0.5 g=6 g$

Number of moles = $\frac{Amount in grams}{molar mass}=\frac{6 \mathrm{g}}{100.088 \mathrm{g}/\mathrm{mole}}=0.06 moles$

Step 5: Explanation Part (d)

Given,

Calcium carbonate in two tablets is $2\times 0.5 g=1 g$

$\text{ Number of mole }=\frac{1 \mathrm{g}}{100.088 \mathrm{g}/\mathrm{mole}}=0.01 moles$

The amount of grams of calcium obtained is,

$0.010\text{ mole }\mathrm{Ca}\times \frac{40.078 \mathrm{g} \mathrm{Ca}}{1.00\text{ mole Ca }}=0.4 \mathrm{g}$

Step 6: Explanation Part (e)

The daily recommended quantity is$1500 mg$

Tums tablets that are needed each day to supply the needed calcium in older women are,

$1500 \mathrm{mg} \mathrm{CaCO}3\times \frac{1 \mathrm{tablet}}{500 \mathrm{mg} \mathrm{CaCO}}=3$

Hence $3$ tablets are required.