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3 years ago

If you keep adding sugar to water and there comes a point that you cannot dissolve any more sugar into it then this is called?

Chemistry

1 answer:

Sliva [168]3 years ago

4 0

Answer:

the answer is letter D, Dilute solution

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29 Which compounds are classified as Arrhenius acids?(1) HCl and NaOH

vitfil [10]

(4) HBr and H2SO4 is the correct answer.
Hope this would help~

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4 years ago

0.5 kg or 0.5 lb which is a larger quantity

masha68 [24]

The correct answer is 0.5 kg If you whant me to explaine pls tell me

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3 years ago

A saline solution contains 0.770 gg of NaClNaCl (molar mass = 58.55 g/molg/mol) in 133 mLmL of solution. Calculate the concentra

lukranit [14]

Answer:

0.104 M

Explanation:

A saline solution contains 0.770 g of NaCl (molar mass = 58.55 g/mol) in 133 mL.

The molar mass of the solute (NaCl) is 58.55 g/mol. The moles corresponding to 0.770 g are:

0.770 g × (1 mol/55.85 g) = 0.0138 mol

The volume of solution is 133 mL. In liters,

133 mL × (1 L/1000 mL) = 0.133 L

The molarity of NaCl is:

M = moles of solute / liters of solution

M = 0.0138 mol / 0.133 L

M = 0.104 M

4 0

3 years ago

Is pizza a element compound homogeneous mixture or heterogeneous mixture?

UNO [17]

Pizza is a heterogeneous mixture Can I get Brainliest??

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3 years ago

G the normal range of the ph of blood is between 7.35 and 7.45; variations beyond this range have significant health implication

Fiesta28 [93]

Answer : the hydrogen ion concentrations for pH = 7.35 and pH = 7.45 are 4.46 x 10⁻⁸ M and 3.54 x 10⁻⁸ M respectively.

When the pH of a solution is less than 7, the hydrogen ion concentration is higher and therefore the solution is acidic.

On the other hand, when the pH of a solution is greater than 7, hydroxide ion concentration is higher and the solution acts as a base.

The normal pH range of blood is given as 7.35 - 7.45 which is greater than 7. That means blood is slight basic in nature.

Let us find hydroxide ion concentration of blood.

$pH + pOH = 14$

$7.35 + pOH = 14$

$pOH = 6.65$

$pOH = - log [OH-]$

$[OH-] = 10^{-6.65}$

$[OH-] = 2.24 \times 10^{-7}$

Ionic product of water is written as,

$[H+] [OH-] = 1 \times 10^{-14}$

Let us plug in the calculated value of [OH-]

$[H+] = \frac{1 \times 10^{-14}}{2.24 \times 10^-7} = 4.46 \times 10^{-8} M$

The hydrogen ion concentration for pH = 7.35 is 4.46 x 10⁻⁸ M

Calculation of [H+] for pH = 7.45

pOH = 6.55

[OH-] = 2.82 x 10⁻⁷

$[H+] = \frac{1 \times 10^{-14}}{2.82 \times 10^-7} = 3.54 \times 10^{-8} M$

Similarly, for pH = 7.45, we get hydrogen ion concentration of 3.54 x 10⁻⁸ M.

8 0

4 years ago