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s2008m [1.1K]
3 years ago
15

Define "Homoglycan" and "Heteroglycan" and give an example of each

Chemistry
1 answer:
lina2011 [118]3 years ago
4 0

Answer:

Polysaccharides, also known as glycans, are the polymers of carbohydrate. These polymers are composed of the monosaccharide monomeric units that are joined together by glycosidic bonds.  

A polysaccharide molecule composed of the same type of monosaccharide units is known as homopolysaccharide or homoglycan.

Example: Cellulose, glycogen, and cellulose.

Whereas, a polysaccharide molecule composed of more than type of monosaccharide is known as heteropolysaccharides or heteroglycans.

Examples: Hyaluronic acid and heparin

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Pure water is 40 percent acid and 60 percent alkaline <br><br> True or false
Verdich [7]
The answer would be true
3 0
3 years ago
Why is sugar considered an organic compound
Sliva [168]
Sugar is considered an organic compound,
Because it is made up a long chain of carbon atoms.
5 0
3 years ago
Empirical formula of a compound composed of 32.1 g potassium (k) and 6.57 g oxygen (o)?
tester [92]

The empirical formula is K₂O.

The empirical formula is the <em>simplest whole-number ratio</em> of atoms in a compound.

The <em>ratio of atom</em>s is the same as the <em>ratio of moles</em>.

So, our job is to calculate the <em>molar ratio</em> of K to O.

Step 1. Calculate the <em>moles of each element </em>

Moles of K = 32.1 g K × (1 mol K/(39.10 g K =) = 0.8210 mol K

Moles of O = 6.57 g O × (1 mol O/16.00 g O) = 0.4106 mol 0

Step 2. Calculate the <em>molar ratio of each elemen</em>t

Divide each number by the smallest number of moles and round off to an integer

K:O = 0.8210:0.4106 = 1.999:1 ≈ 2:1

Step 3: Write the <em>empirical formula </em>

EF = K₂O

5 0
3 years ago
An analytical chemist weighs out 0.093g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with
Kamila [148]

Answer:

The molar mass of the unknown acid is 89 g/mol

Explanation:

<u>Step 1:</u> The balanced equation

HA(aq) + NaOH(aq) → NaA(aq) + H2O(l)

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

<u>Step 2:</u> Data given

Mass of the acid = 0.093 grams

volume = 250 mL

titrates with 0.16 M NaOH

adds 6.5 mL NaOH

<u>Step 3: </u>Calculate moles of NaOH

We know the concentration and volume of NaOH needed to neutralize the acid.

By determining the moles of NaOH in that volume in liters (95.9mL=0.0959L), the moles of acid in the original sample can be determined from the reaction stoichiometry.

Moles = Molarity * Volume

Moles = 0.16 M * 0.0065 L

Moles = 0.00104 moles NaOH

<u>Step 4: </u>Calculate moles of the unknown acid:

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

For 0.00104 moles NaOH we have 0.00104 moles of HA

<u>Step 5: </u>Calculate the molar mass of the acid

Molar mass Ha = Mass Ha / moles Ha

Molar mass Ha = 0.093 grams / 0.00104 moles

Molar mass Ha = 89.42 g/mol ≈89 g/mol

The molar mass of the unknown acid is 89 g/mol

3 0
3 years ago
J. A gas has a volume of 12 L at 200°C with 6.0 atm.
White raven [17]

Gay Lussac's Law

\tt \dfrac{P_1}{T_1}=\dfrac{P_2}{T_2}

Convert:

200°C = 200 + 273 = 473 K

50°C = 50 + 273 = 323 K

Input the value:

\tt \dfrac{6}{473}=\dfrac{P_2}{323}\\\\P_2=4.097~atm

4 0
2 years ago
Read 2 more answers
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