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4 years ago

Determine the hydroxide ion concentration in a solution that is 0.018 m naoh.

1 answer:

5 0

As we know, NaOH is a strong Base and completely dissociates in water as given below,

NaOH + H₂O → Na⁺ ₍aq₎ + OH⁻ ₍aq₎

So, the concentration of OH⁻ Ions will be the same as that the concentration of NaOH i.e. 0.018 M.
So,
[OH⁻] = 0.018 M

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What type of bonding will be present in the oxyde of the element with atomic number 1?

Bad White [126]

Answer:

Element with the atomic number 1 is hydrogen whose oxide is water having covalent bonds.

Explanation:

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3 years ago

How many liters of the antifreeze ethylene glycol [CH2(OH)CH2(OH)] would you add to a car radiator containing 6.50 L of water if

sergeinik [125]

16 = m x 1.86
m = 8.60 = moles solute / 6.50 Kg

moles solute = 55.9

mass solute = 55.9 x 62.068 g/mol=3470 g

V = 3479/ 1.11 =3126 mL= 3.13 L

delta T = 8.60 x 0.512 =4.40
boling point = 104.4 °C

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3 years ago

Read 2 more answers

What is the general formula of alkene?

Svetradugi [14.3K]

The general formula for the alkenes is C nH 2n

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3 years ago

A particular substance has a measured solubility in water of 3.6g/1.0L. How much of the substance can be dissolved in 650 L of w

harkovskaia [24]

I believe the correct answer is 2340g of a particular substance will be dissolved in 650 L of H2O. Hope I was helpful in some way. Thanks. Peace.

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4 years ago

How many grams of chlorine gas are present in a 150. liter cylinder of chlorine held at a pressure of 1.00 atm and 0. °C? Group

OlgaM077 [116]

Answer:

474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P*V = n*R*T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

In this case:

P= 1.00 atm
V= 150 L
n= ?
R= 0.082 $\frac{atm*L}{mol*K}$
T= 0 C= 273 K

Replacing:

1.00 atm* 150 L= n*0.08206 $\frac{atm*L}{mol*K}$ *273 K

Solving:

$n=\frac{1.00 atm* 150 L}{0.08206 \frac{atm*L}{mol*K}*273 K}$

n= 6.69 moles

Being Cl= 35.45 g/mole, the molar mass of chlorine gas is:

Cl₂=2*35.45 g/mole= 70.9 g/mole

So if 1 mole has 70.9 grams, 6.69 moles of the gas, how much mass does it have?

$mass=\frac{6.69 moles*70.9 grams}{1 mole}$

mass= 474.321 grams ≅ 474 grams

474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C

4 0

3 years ago