Why are city streets so vital to the functioning of a city, as well as the people living within it?

What forces typically hold ionic solids together?

just olya [345]

Answer: D. Electrostatic forces

Explanation:

7 0

3 years ago

1718 l of a 0.3556-m c3h7oh solution is diluted to a concentration of 0.1222 m, what is the volume of the resulting solution

Agata [3.3K]

Answer : The volume of the resulting solution will be 0.4999 L.

Explanation : As the two molar concentration of the $C_{3} H_{7}OH$ solution are given and one of the volume concentration needs to be found.

So, according to the formula :- $m_{1}V_{1} = m_{2}V_{2}$

And here if we consider $V_{1}$ as 0.1718 L moles and $m_{1}$ as 0.3556 moles then we need to find $V_{2}$ as $m_{2}$ is given as 0.1222 moles.
Hence on solving the formula we get,

$V_{2}$ = (0.1718 X 0.3556) / 0.1222 = 0.4999 L

5 0

4 years ago

Explain why it is important that there be no gaps around the edges of the filter paper during a vacuum filtration

lesantik [10]

Vacuum filtration is more efficient and faster than filtration by the gravity method. But the set up of the vacuum filtration must be precise. Vacuum filtration is done under very reduced pressure hence there should be no gaps around the edges of the filter paper. For a vacuum to be effective there must be no hole or gap in the equipment. Under vacuum conditions air is removed and the pressure is lowered. If there is gap then air would be continuously supplied and it would be difficult to remove air completely.

4 0

3 years ago

Why is it important that there is only a small amount of water in the beaker

natita [175]

Answer:

because too much can neutralise the results

4 0

4 years ago

Read 2 more answers

When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced.

sp2606 [1]

Answer:

Mass of CaCl₂ = 20 g

CaCO is presewnt in excess.

Mass of of CaCO₃ remain unreacted = 7.007 g

Explanation:

Given data:

Mass of calcium carbonate = 25 g

Mass of hydrochloric acid = 13.0 g

Mass of calcium chloride produced = ?

Chemical equation:

CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂

Number of moles of CaCO₃:

Number of moles of CaCO₃ = Mass /molar mass

Number of moles of CaCO₃= 25.0 g / 100.1 g/mol

Number of moles of CaCO₃ = 0.25 mol

Number of moles of HCl:

Number of moles of HCl = Mass /molar mass

Number of moles of HCl = 13.0 g / 36.5 g/mol

Number of moles of HCl = 0.36 mol

Now we will compare the moles of CaCl₂ with HCl and CaCO₃ .

CaCO₃ : CaCl₂

1 : 1

0.25 : 0.25

HCl : CaCl₂

2 : 1

0.36 : 1/2 × 0.36 = 0.18 mol

The number of moles of CaCl₂ produced by HCl are less it will be limiting reactant.

Mass of CaCl₂ = moles × molar mass

Mass of CaCl₂ =0.18 mol × 110.98 g/mol

Mass of CaCl₂ = 20 g

The calcium carbonate is present in excess.

HCl : CaCO₃

2 : 1

0.36 : 1/2 × 0.36 = 0.18 mol

So, 0.18 moles react with 0.36 moles of HCl.

The moles of CaCO₃ remain unreacted = 0.25 -0.18

The moles of CaCO₃ remain unreacted = 0.07 mol

Mass of of CaCO₃ remain unreacted = Moles × molar mass

Mass of of CaCO₃ remain unreacted = 0.07 mol × 100.1 g/mol

Mass of of CaCO₃ remain unreacted = 7.007 g

7 0

3 years ago