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1 year ago

Explain how a solution can be both dilute and saturated.

Chemistry

2 answers:

katrin2010 [14]1 year ago

7 0

Answer:

A solution can be diluted and saturated at the same time depending on the solubility of the solute.

Explanation:

A dilute solution is when the amount of solute is in a small amount of solvent, and a saturated solution occurs when the solvent contains the maximum amount of solute that can be dissolved at a specific temperature.

These 2 concepts can occur at the same time depending on the solubility of the solute, for example a saturated solution of CaCO3 will be diluted because the compound is very poorly soluble in the solvent.

svlad2 [7]1 year ago

4 0

Dilution is when you decrease the concentration of a solution by adding a solvent. As a result, if you want to dilute salt water, just add water. ... Add more solute until it quits dissolving. That point at which a solute quits dissolving is the point at which it's saturated.

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A student pours exactly 26.9 mL of HCl acid of unknown molarity into a beaker. The student then adds 2 drops of the indicator an

Assoli18 [71]

a.
Acids react with bases and give salt and water and the products.

Hence, HCl reacts with NaOH and gives NaCl salt and H₂O as the products. The reaction is,
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

To balance the reaction equation, both sides hould have same number of elements.

Left hand side, Right hand side,
H atoms = 2 H atoms = 2
Cl atoms = 1 Cl atoms = 1
Na atoms = 1 Na atoms = 1
O atoms = 1 O atoms = 1

Hence, the reaction equation is already balanced.

b.
Molarity (M)= moles of solute (mol) / Volume of the solution (L)

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

Molarity of NaOH = 0.13 M
Volume of NaOH added = 43.7 mL
Hence, moles of NaOH added = 0.13 M x 43.7 x 10⁻³ L
= 5.681 x 10⁻³ mol

Stoichiometric ratio between NaOH and HCl is 1 : 1

Hence, moles of HCl = moles of NaOH
= 5.681 x 10⁻³ mol

5.681 x 10⁻³ mol of HCl was in 26.9 mL.

Hence, molarity of HCl = 5.681 x 10⁻³ mol / 26.9 x 10⁻³ L
= 0.21 M

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2 years ago

How many moles are in 1.50 g of ethylamine, ch3ch2nh2?

zavuch27 [327]

Mass = mass/molar mass of ch3ch2nh2
the molar mass of CH3CH2NH2 = 12 +(1x3)+12+(1 x2)+14+(1x2) =45 g/mol

moles is therefore = 1.50g /45g/mol = 0.033 moles

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1 year ago

Read 2 more answers

If Maria winks exactly 5 times every minute while she is awake and she sleeps exactly 8 hours a day, how many times does Maria w

irina1246 [14]

24 minus 8 is 16
5 times 60 is 300
300 times 16 is 4800.
She winks 4800 times a day

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1 year ago

If a large marshmallow has a volume of 2.50 i n 3 and density of 0.242 g/c m 3 , how much would it weigh in grams? 1 i n 3 =16.3

Illusion [34]

Density of a substance is defined as the mass of the substance divided by the volume.

Density of the substance= 0.242 g cm⁻³

volume of the substance= 2.50 in³

As, 1 in³= 16.39 cm³

So, 2.50 in³= 16.39× 2.50 cm³=40.97 cm³

As ,

$Density=\frac{mass}{volume}$

Mass=volume ×Density

Mass=40.97 × 0.242

Mass=9.916 g.

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1 year ago

At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must be added at constant temper

fgiga [73]

Answer:

We have to add 2.30 L of oxygen gas

Explanation:

Step 1: Data given

Initial volume = 4.00 L

Number of moles oxygen gas= 0.864 moles

Temperature = constant

Number of moles of oxygen gas increased to 1.36 moles

Step 2: Calculate new volume

V1/n1 = V2/n2

⇒V1 = the initial volume of the vessel = 4.00 L

⇒n1 = the initial number of moles oxygen gas = 0.864 moles

⇒V2 = the nex volume of the vessel

⇒n2 = the increased number of moles oxygen gas = 1.36 moles

4.00L / 0.864 moles = V2 / 1.36 moles

V2 = 6.30 L

The new volume is 6.30 L

Step 3: Calculate the amount of oxygen gas we have to add

6.30 - 4.00 = 2.30 L

We have to add 2.30 L of oxygen gas

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1 year ago