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kotegsom [21]
3 years ago
6

A solution is highly concentrated if there is:

Chemistry
1 answer:
yuradex [85]3 years ago
3 0
TO be saturated you need an amount of solvent that will not dissolve anymore into the solution.  So, the best answer from the list is C
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I would appreciate your help! Due today! ( I don't know if this is even chemistry)
Vinil7 [7]

Answer:

6+69

Explanation:

6 0
3 years ago
Read 2 more answers
Reduce the following molecular formulas to empirical formulas. Please help!
zvonat [6]
This is done by reducing each number by a common factor for each formula.

C3H6O6- all can be divided by 3 -> CH3O3 (you don't have to put a 1 for C, only if your teacher requests it. It is generally understood if not written)

H2O2- all can be divided by 2 -> H1O1 (had to put the 1's bc of the unintended language) 

C8H8S2- all can be divided by 2 -> C4H4S 

P5O15- all can be divided by 5- PO3

*****it is important to note that <em>all </em>numbers in the molecular formula are divided by the same thing to reduce them. decimals are <em>never </em>used in empirical formulas, only whole numbers.*****
3 0
3 years ago
You are given 1.000 grams of hydrated Magnesium Sulfate (MgSO4*XH20). You place it into a crucible and heat it up past 100 C so
adelina 88 [10]

Answer:

MgSO4. 7H2O

There are seven water molecules attached to the hydrated salt.

Explanation:

From the equation;

Number of moles of hydrated salt = number of moles of anhydrous salt, we obtain:

Mass of hydrated salt/ molar mass of hydrated salt = mass of anhydrous salt/ molar mass of anhydrous salt

From the question;

Mass of hydrated salt = 1.000g

Molar mass of hydrated salt = 120.366 +18x gmol-1

Mass of anhydrous salt= 0.488g

Molar mass of anhydrous salt= 120.366 gmol-1

Substituting into the equation above;

1.000/120.366 +18x = 0.488/120.366

1.000/120.366 +18x = 0.004

1.000= 0.004 (120.366 +18x)

1.000= 0.48 + 0.072x

1.000 - 0.48 = 0.072x

0.52= 0.072x

x= 0.52/0.072

x=7

Therefore the hydrated salt is MgSO4. 7H2O

3 0
3 years ago
9.50 L of Fluorine gas at STP reacts with 6.945x1024 formula units of Chromium (VI) chloride.
lorasvet [3.4K]

Answer:

Again please specify your question, you still haven't indicated what you want to be solved.

by formula units I assume you mean atoms?

I'll edit my answer accordingly if you could specify down in the comments.

8 0
3 years ago
When the following oxidation-reduction occurs, what is the balanced reduction half-reaction after the electrons in both half rea
Lostsunrise [7]

Answer :  The balanced reduction half-reaction is:

3Cu^{2+}+6e^-\rightarrow 3Cu

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

The given balanced redox reaction is :

Al(s)+Cu^{2+}(aq)\rightarrow Al^{3+}(aq)+Cu(s)

The half oxidation-reduction reactions are:

Oxidation reaction : Al\rightarrow Al^{3+}+3e^-

Reduction reaction : Cu^{2+}+2e^-\rightarrow Cu

In order to balance the electrons, we multiply the oxidation reaction by 2 and reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

Oxidation reaction : 2Al\rightarrow 2Al^{3+}+6e^-

Reduction reaction : 3Cu^{2+}+6e^-\rightarrow 3Cu

The balanced redox reaction will be:

2Al(s)+3Cu^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Cu(s)

Thus, the balanced reduction half-reaction is:

3Cu^{2+}+6e^-\rightarrow 3Cu

6 0
3 years ago
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