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Korvikt [17]
3 years ago
6

10 POINT

Chemistry
1 answer:
MAVERICK [17]3 years ago
8 0
the correct answer is B
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4. Jake surveyed his 25 classmates on their favorite flavor of
Eddi Din [679]

Answer:

J

Explanation:

In total there are 25 students. If you add up all the other students who liked flavors other than strawberry twist you will get 14. That means 14/25 students did not favor strawberry twist, while the other 11/25 did.

4 0
3 years ago
sodium hydroxide, NaOH , is dissolved in water to make up a solution that is 1.58× 10 −5 M in NaOH . What is the pH
mars1129 [50]

Answer:

pH = 9.2

Explanation:

pH+pOH=14

But pOH= -log[OH]= -log[1.58×10^-5]= 4.8

We can now say

4.8+pH= 14

pH= 14-4.8= 9.2

8 0
3 years ago
Can someone help me with this??
zloy xaker [14]

゚+*:ꔫ:*﹤  ﹥*:ꔫ:*+゚Answer:゚+*:ꔫ:*﹤  ﹥*:ꔫ:*+゚

The following: Jupiter, Saturn, Uranus, or Neptune.

゚+*:ꔫ:*﹤  ﹥*:ꔫ:*+゚Explanation:゚+*:ꔫ:*﹤  ﹥*:ꔫ:*+゚

any of the planets Jupiter, Saturn, Uranus, and Neptune whose orbits lie beyond the asteroid belt.

5 0
2 years ago
Read 2 more answers
How many grams of fluorine are contained in 8 molecules of boron trifluoride?
Lelu [443]
<h3>Answer:</h3>

             7.57 × 10⁻²² g of F

<h3>Solution:</h3>

Data Given:

                 Number of Molecules  =  8

                 M.Mass of BF₃ =  67.82 g.mol⁻¹

                 Mass of Fluorine atoms  =  ?

Step 1: Calculate Moles of BF₃

           Moles  =  Number of Molecules ÷ 6.022 × 10²³ Molecules.mol⁻¹

Putting value,

            Moles  =   8 Molecules ÷ 6.022 × 10²³ Molecules.mol⁻¹

            Moles  =  1.33 × 10⁻²³ mol

Step 2: Calculate Mass of BF₃:

                   Moles  =  Mass ÷ M.Mass

Solving for Mass,

                   Mass  =  Moles × M.Mass

Putting values,

                   Mass  =  1.33 × 10⁻²³ mol × 67.82 g.mol⁻¹

                   Mass  =  9.0 × 10⁻²² g

Step 3: Calculate Mass of Fluorine Atoms:

As,

                         67.82 g BF₃ contains  =  57 g of F

So,

                    9.0 × 10⁻²² g will contain  =  X g of F

Solving for X,

                       X =  (9.0 × 10⁻²² g × 57 g) ÷ 67.82 g

                        X  =  7.57 × 10⁻²² g of F

4 0
3 years ago
Read 2 more answers
A chemist prepares a solution of magnesium chloride MgCl2 by measuring out 49.mg of MgCl2 into a 100.mL volumetric flask and fil
Flura [38]

Answer:  Molarity of Cl^- anions in the chemist's solution is 0.0104 M

Explanation:

Molarity : It is defined as the number of moles of solute present per liter of the solution.

Formula used :

Molarity=\frac{n\times 1000}{V_s}

where,

n= moles of solute

Moles=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{0.049g}{95g/mol}=5.2\times 10^{-4}moles  

V_s = volume of solution in ml = 100 ml

Now put all the given values in the formula of molarity, we get

Molarity=\frac{5.2\times 10^{-4}moles\times 1000}{100ml}=5.2\times 10^{-3}mole/L

Therefore, the molarity of solution will be 5.2\times 10^{-3}mole/L

MgCl_2\rightarrow Mg^{2+}+2Cl^-

As 1 mole of MgCl_2 gives 2 moles of Cl^-

Thus 5.2\times 10^{-3}  moles of MgCl_2 gives =\frac{2}{1}\times 5.2\times 10^{-3}=0.0104

Thus the molarity of Cl^- anions in the chemist's solution is 0.0104 M

6 0
3 years ago
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