All categories

2 years ago

How does solubility differ between small versus large carbohydrates? Explain.

Chemistry

1 answer:

EleoNora [17]2 years ago

5 0

Answer with Explanation:

Small and large carbohydrates have diverse structural properties. Such property allow them to have different solubility.

Solubility is a chemical property of a substance that allows it to dissolve in a given solvent.

Carbohydrates are made up of "monosaccharides." These are simple sugars and are considered small carbohydrates. On the contrary, "polysaccharide" is an example of a large carbohydrate. Monosaccharides are soluble in water while many polysaccharides are not soluble in water.

The high solubility of monosaccharides is mainly due to the presence of hydroxide (OH) groups. These groups are always ready to bond with water (H₂O). Many polysaccharides are not soluble in water because of intermolecular interactions that prevents it from binding with water. Its dissolution process is different when compared to the smaller molecules.

So, this explains the answer.

You might be interested in

How many moles of copper are there in 6.93 g of copper sample pls be quick

Alex_Xolod [135]

Molar mass of copper=63.5g/mol
Given mass=6.93g

$\\ \sf\longmapsto No\:of\;moles=\dfrac{Given\:mass}{Molar\:mass}$

$\\ \sf\longmapsto No\:of\:moles=\dfrac{6.93}{63.5}$

$\\ \sf\longmapsto No\:of\:moles=0.109\approx 1.11moles$

7 0

1 year ago

Read 2 more answers

Calculate the mass of oxygen in 30 g of CH NH COOH?

Naya [18.7K]

Molar mass of CH2NH2COOH - 75

Given mass of CH2NH2COOH - 30

Moles of CH2NH2COOH = Given mass/ Molar mass

moles of CH2NH2COOH = 30/75 = 0.4 mol

One mole of CH2NH2COOH contains 32 gram of oxygen

0.4 mole of CH2NH2COOH will contain = 0.4 × 32= 12.8 g of oxygen

Answer- the mass of oxygen in 30 g of CH2NH2COOH is 12.8 gram!

7 0

2 years ago

hich quantity describes how spread out a set of data is? O A. Standard deviation O B. Percent error O C. Line of best fit D. Mea

juin [17]

The answer to this is B.

6 0

3 years ago

What is the new pressure of 150 mL of a gas that is compressed to 50 mL when the original pressure was 3.0 ATM and the temperatu

Arisa [49]

Answer:

$\boxed {\boxed {\sf P_2= 9 \ atm}}$

Explanation:

Since the temperature is held constant, we only need to focus on the volume and pressure. We will use Boyle's Law, which states the volume of a gas is inversely proportional to the pressure. The formula is:

$P_1V_1=P_2V_2$

Originally, the gas had a volume of 150 milliliters and a pressure of 3.0 atmospheres. We can substitute these values into the left side of the equation.

$3.0 \ atm * 150 \ mL = P_2V_2$

The original gas was compressed to a volume of 50 milliliters, but we don't know the volume.

$3.0 \ atm *150 \ mL= P_2 * 50 \ mL$

Now, we need to solve for the new pressure (P₂). Multiply on the left side first.

$450 \ atm*mL= P_2 * 50 \ mL$

Since we are solving for the pressure, we need to isolate the variable. It is being multiplied by 50 mL. The inverse of multiplication is division. Divide both sides by 50 mL.

$\frac{450 \ atm*mL}{50 \ mL}= \frac{P_2 * 50 \ mL}{50 \ mL}$

$\frac{450 \ atm*mL}{50 \ mL}= P_2$

The units of milliliters will cancel.

$\frac{450 \ atm}{50 }= P_2$

$9 \ atm =P_2$

The new pressure is 9 atmospheres.

8 0

2 years ago

How many mL of 4.0% Mg(NO3)2 solution would contain 1.2 g of magnesium nitrate?

galina1969 [7]

4.0 % in mass per volume :

4.0 g ---------- 100 mL
1.2 g ---------- ( volume )

Volume = 1.2 x 100 / 4.0

Volume = 120 / 4.0

= 30 mL

hope this helps!

8 0

3 years ago