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University of Maine

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Problem 127

Citric acid (right) is concentrated in citrus fruits and plays a central metabolic role in nearly every animal and plant cell. (a) What are the molar mass and formula of citric acid? (b) How many moles of citric acid are in 1.50 qt of lemon juice $(d=1.09 \mathrm{g} / \mathrm{mL})$ that is 6.82$\%$ citric acid by mass?

Answer

a)

$\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$

$\operatorname{Mr}\left(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\right)=192,12 \mathrm{g} / \mathrm{mol}$

b)

$\mathrm{n}($ citric acid $)=0,55 \mathrm{mol}$

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## Discussion

## Video Transcript

the image given is what's called the structural formula, and it tells us the atoms present on a molecule as well as how they're connected. So to write the molecular formula, we simply add up the different elements. You can see that there's carbon, and if you count them, there are six the blue or the hydrogen. 12345678 And finally the oxygen's. The reds are seven, so the molecular formula is C six, h, 807 and the molar masses simply adding up the individual more masses and multiplying by how Muneer present so six times the moulder massive carbon I just found on the periodic table, plus eight times the molar mass of hydrogen also on the periodic table, and seven times 15.999 which is more math of oxygen. This equals 192 0.12 grams per mole. So that's the molar mass, and we can use this information to make a conversion about different types of solutions. If we have, for example, 1.5 quarts of a solution, that's 6.8% citric acid, 6.82%. We can determine how many moles of the actual citric acid or present. We also know the density of the solution is 1.9 grams per mil. We'll start with their given quantity and we'll convert to milliliters using the conversion. We can then find grams using the density which we can then find grams of the citric acid and using the percentage. And finally we confined the moles using molar mass. There are 946.35 milliliters in every court and the density is 109 grams per milliliter. And we know that we need to multiply this fire percent 4.0 682 This gives us 105 0.7 grams of C six h, 807 to change two moles. We use the molar mass that we found a bug and we divide for everyone. Mole, there are 100 and 92.12 grams or our final answer is 0.549 moles of citric acid

## Recommended Questions

Citric acid is one component of some soft drinks. Suppose that 2.00 L of solution are made from $150 .$ mg of citric acid, $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$

a. What is the molar mass of citric acid?

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Citric acid, which can be obtained from lemon juice, has the molecular formula $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7} .$ A $0.250-\mathrm{g}$ sample of citric acid dissolved in $25.0 \mathrm{mL}$ of water requires $37.2 \mathrm{mL}$. of $0.105 \mathrm{M} \mathrm{NaOH}$ for complete neutralization. How many acidic hydrogens per molecule does citric acid have?

Citric acid, which can be obtained from lemon juice, has the molecular formula $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$ . A 0.250 -g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

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A $1.37-M$ solution of citric acid $\left(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)$ in water has a density of $1.10 \mathrm{g} / \mathrm{cm}^{3} .$ Calculate the mass percent, molality, mole fraction, and normality of the citric acid. Citric acid has three acidic protons.

Citric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3) . (a) Calculate the pH of a 0.040$M$ solution of citric acid. (b) Did you have to make any approximations or assumptions in completing your calculations? (c) Is the concentration of citrate ion $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}^{3-}\right)$ equal to, less than, or greater than the $\mathrm{H}^{+}$ ion concentration?

Citric acid is responsible for the tartness of citrus fruits, especially lemons and limes.

a. What is the molecular formula for citric acid?

b. How many lone pairs are present?

c. Draw a skeletal structure.

d. How many $sp^2$ hybridized carbons are present?

e. What orbitals are used to form each indicated bond ([1]-[4])?

What is the percent composition of citric acid, an organic acid, commonly found in citrus fruits, whose structure is shown in the nearby margin? (Gray $=\mathrm{C}$ red $=\mathrm{O}, \mathrm{H}=$ ivory.)

Citric acid, the compound responsible for the sour taste of lemons, has the elemental composition: $\mathrm{C}, 37.51 \% ; \mathrm{H}$ $4.20 \% ; \mathrm{O}, 58.29 \% .$ Calculate the empirical formula of citric acid.

Citric acid has three dissociable hydrogens. When 5.00 $\mathrm{mL}$ of 0.64 $\mathrm{M}$ citric acid and 45.00 $\mathrm{mL}$ of 0.77 $\mathrm{M} \mathrm{NaOH}$ are mixed at an initial temperature of $26.0^{\circ} \mathrm{C}$ , the temperature rises to $27.9^{\circ} \mathrm{C}$ as the citric acid is neutralized. The combined mixture has a mass of 51.6 $\mathrm{g}$ and a specific heat of 4.0 $\mathrm{J} /\left(\mathrm{g} \cdot^{\circ} \mathrm{C}\right) .$ Assuming that no heat is transferred to the surroundings, calculate the enthalpy change for the reaction of 1.00 $\mathrm{mol}$ of citric acid in $\mathrm{kJ} .$ Is the reaction exothermic or endothermic?