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3 years ago

I need help on science lol

Chemistry

2 answers:

jeyben [28]3 years ago

8 0

Answer: C

Explanation: i think i looked at my notes from 3 months ago when i did this i think C is the best choice let me know after ypu take the test

lara [203]3 years ago

6 0

Answer:

chicken and macaroni

Explanation:

cus

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Read these scenarios about two different countries

Debora [2.8K]

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3 years ago

How does carbonic acid work to maintain blood pH? (Select all that apply.) Check All That Apply When blood is too basic, carboni

Vlad1618 [11]

Answer:

When blood is too basic, carbonic acid can ionize to bicarbonate and H+ ions, adding H+ ions to the blood.

When blood becomes too acidic, bicarbonate combines with extra H+ ions to form carbonic acid, removing H+ ions from the blood.

Carbonic acid can raise or lower the pH of blood.

Explanation:

A buffer is a solution that resists changes to its pH when small quantities of acids or bases are added to it. The human blood serves as a buffer as it contains a buffer of carbonic acid (H2CO3) and bicarbonate anion (HCO3-) which serves to maintain blood pH between 7.35 and 7.45. Other buffering systems in blood exist such as the Hydrogen ion and oxygen gas which affects oxygen binding to haemoglobin, however the carbonic-acid-bicarbonate buffer is the most important buffer for maintaining acid-base balance in the blood.

A buffer solution is made up of an acid and its conjugate base or a base and its conjugate acid. For carbonic acid-bicarbonate buffer, carbonic acid serves as the acid while bicarbonate serves as the base. When a little quantity of a base as hydroxide ions is added to a buffer, the acid reacts with it and remove it from the solution. On the other hand, when a little quantity of an acid as hydrogen ions are added to a buffer, the conjugate base reacts with it and remove it from the solution, thus keeping the pH of the solution fairly constant.

In the carbonic acid-bicarbonate buffer:

When blood is too basic, carbonic acid can ionize to bicarbonate and H+ ions, adding H+ ions to the blood.

When blood becomes too acidic, bicarbonate combines with extra H+ ions to form carbonic acid, removing H+ ions from the blood.

Thus, carbonic acid can raise or lower the pH of blood.

3 0

3 years ago

Explain the relationship between heat transfer and calorimetry. Justify your response in two or more complete sentences.

babymother [125]

Calorimetry is the measurement of the quantity of heat in a substance. It is a method that is used to measure the energy content of food. It is also used to measure the specific heat of substances.

8 0

3 years ago

A molecule contains 23.24 g iodine (I),

gavmur [86]

Convert each amount of grams into moles:

I: 23.24g x 1 mol / 126.90g = 0.1831 mol I

C: 2.198 x 1 mol / 12.01g = 0.1830 mol C

N: 2.562 x 1 mol / 14.01g = 0.1829 mol N

Each element has roughly the same amount of moles, which means the whole number ratio between the elements is 1:1:1

Therefore the empirical formula is ICN

7 0

3 years ago

Hydrogen Peroxide, H2O2, in the presence of a catalyst decomposes into water and oxygen gas. How many L of O2 at STP are produce

Korolek [52]

Answer:

There is 11.2 L of O2 produced

Explanation:

Step 1: Data given

Molar mass of H2O2 = 34.01 g/mol

Molar mass of O2 = 32 g/mol

Mass of H2O2 = 34.0 grams

Step 2: The balanced reaction

2H2O2 → 2H2O + O2

Step 3: Calculate number of moles H2O2

Moles H2O2 = Mass H2O2 / Molar mass H2O2

Moles H2O2 = 34 grams / 34.01 g/mol

Moles H2O2 = 1 mol

Step 4: Calculate the number of moles at the equilibrium

Initial number of moles H2O2 = 1 mol

Initial number of mol H2O and O2 = 0 mol

Since the mol ratio H2O2 H2O O2 is 2:2:1

There will react x mol of H2O2; X mol of H2O and 0.5 x mol of O2

At the equilibrium, H2O2 has (1-x) mol. Since it's decomposed into H2O and O2, we know x =1 mol

At the equilibrium, there is 1 mol H2O and 0.5 mol O2

Under STP, 1 mol of gas has a volume of 22.4 L

This means 0.5 moles of O2 has a volume of 22.4*0.5 = 11.2 L

There is 11.2 L of O2 produced

4 0

3 years ago