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swat32
2 years ago
6

What pH must organisms maintain

Chemistry
2 answers:
vazorg [7]2 years ago
7 0
It's different for each organ. So in the stomach its gotta be acidic and in your blood its gotta be neutral
MA_775_DIABLO [31]2 years ago
5 0
6.5-7.5 i believe was right
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A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The
iVinArrow [24]

Answer:

[NH₃]  → 3.24 M  

Explanation:

Our solute: Ammonia

Our solvent: Water

Solution's mass = Mass of solute + Mass of solvent

Solution's mass = 15 g + 250 g = 265g

We use density to determine, the volume.

D = mass /volume → Volume = m / D →  265 g /0.974 g/mL = 272.07 mL.

We convert the mL to L → 272.07 mL . 1L /1000mL = 0.27207 L

To determine molarity we need the moles of solute in 1 L of solution.

Moles of solute are: 15g / 17g/mol = 0.882 moles

[NH₃] = 0.882mol /0.27207 L → 3.24 M  

3 0
3 years ago
A student obtains the following data: Mass of empty, dry graduated cylinder: 21.577 g Volume added of NaCl solution: 4.602 mL Ma
klasskru [66]

<u>Answer:</u> The density of NaCl solution is 3.930 g/mL

<u>Explanation:</u>

We are given:

Mass of cylinder, m_1 = 21.577 g

Mass of NaCl and cylinder combined, M = 39.664 g

Mass of NaCl, m_2 = (M-m_1)=(39.664-21.577)g=18.087g

To calculate density of a substance, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

We are given:

Mass of NaCl = 18.087 g

Volume of NaCl solution = 4.602 mL

Putting values in above equation, we get:

\text{Density of NaCl}=\frac{18.087g}{4.602mL}\\\\\text{Density of NaCl}=3.930g/mL

Hence, the density of NaCl solution is 3.930 g/mL

7 0
2 years ago
Solid solutions that are mixtures of elements with metallic properties are known as_____
marshall27 [118]
Alloys. hope this helps.
4 0
2 years ago
EXTRA POINTSSS 1. A solution at 25 degrees Celsius is 1.0 × 10–5 M H3O+. What is the concentration of OH– in this solution?
AlekseyPX

Answer:

Concentration of OH⁻:

1.0 × 10⁻⁹ M.

Explanation:

The following equilibrium goes on in aqueous solutions:

\text{H}_2\text{O}\;(l)\rightleftharpoons \text{H}^{+}\;(aq) + \text{OH}^{-}\;(aq).

The equilibrium constant for this reaction is called the self-ionization constant of water:

K_w = [\text{H}^{+}]\cdot[\text{OH}^{-}].

Note that water isn't part of this constant.

The value of K_w at 25 °C is 10^{-14}. How to memorize this value?

  • The pH of pure water at 25 °C is 7.
  • [\text{H}^{+}] = 10^{-\text{pH}} = 10^{-7}\;\text{mol}\cdot\text{dm}^{-3}
  • However, [\text{OH}^{-}] = [\text{H}^{+}]=10^{-7}\;\text{mol}\cdot\text{dm}^{-3} for pure water.
  • As a result, K_w = [\text{H}^{+}] \cdot[\text{OH}^{-}] = (10^{-7})^{2} = 10^{-14} at 25 °C.

Back to this question. [\text{H}^{+}] is given. 25 °C implies that K_w = 10^{-14}. As a result,

\displaystyle [\text{OH}^{-}] = \frac{K_w}{[\text{H}^{+}]} = \frac{10^{-14}}{1.0\times 10^{-5}} = 10^{-9} \;\text{mol}\cdot\text{dm}^{-3}.

8 0
3 years ago
What are the names of the components (each shown with a leader and a line) of a circuit shown in the diagram? Please help!!!!
alekssr [168]
Maybe: Battery, wire, lamp and switch
6 0
2 years ago
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