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Karolina [17]
3 years ago
12

Assume a density of water of 1.00 g/mL, and calculate the mass of water in the solution

Chemistry
1 answer:
tiny-mole [99]3 years ago
5 0

Answer:

1g or 10^-3kg

Explanation:

as you know , the density =mass \volume

so  you have the mass from the number it self

<h2>\frac{1g}{1 ml} so from this equation, you will get 1 g and you can to SI to be 10^{-3}kg</h2>
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A food web is a diagram that shows how different food chains connect. true or false​
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Answer:

true

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2 years ago
Which of the following bonds is most popular?<br> C-C,C-N,C-O,C-H
Akimi4 [234]

The answer is C-O

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4 0
3 years ago
(Help would be greatly appreciated) What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution
luda_lava [24]

Answer:

7.67

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4 0
3 years ago
The densities of gases a, b, and c at stp are 1.25 g/l, 2.86 g/l and 0.714 g/l, respectively. calculate the molar mass of each s
kicyunya [14]
The  molar  mass  of    a, b and  c at  STP is calculated  as  below

At  STP  T  is always=   273 Kelvin and ,P= 1.0 atm 

by  use of  ideal  gas  equation  that  is  PV =nRT
n(number   of moles) = mass/molar mass  therefore  replace   n  in  the  ideal   gas  equation

that  is Pv = (mass/molar mass)RT
multiply  both side  by molar  mass  and  then  divide  by  Pv  to  make  molar mass the  subject of the  formula

that is  molar  mass =  (mass x RT)/ PV

 density is always = mass/volume

therefore  by  replacing  mass/volume  in   the equation  by  density the equation
molar  mass=( density  xRT)/P  where R  =  0.082 L.atm/mol.K

the  molar mass  for  a
= (1.25 g/l  x0.082 L.atm/mol.k  x273k)/1.0atm = 28g/mol

the molar  mass of b
=(2.86g/l  x0.082L.atm/mol.k   x273  k) /1.0  atm  = 64  g/mol

the molar  mass of c

=0.714g/l  x0.082  L.atm/mol.K  x273 K) 1.0atm= 16 g/mol

therefore  the 
   gas  a  is  nitrogen N2   since 14 x2= 28 g/mol
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  gas c =   methaneCH4  since  12+(1x4) = 16 g/mol


8 0
2 years ago
Determine the pH of a 5x10^-4 M solution of Ca(OH)2
miss Akunina [59]
Ca(OH)₂ ==> Ca²⁺ + 2 OH<span>-   

Ca(OH)</span>₂ is <span>strong Bases</span><span>

</span>Therefore,  the [OH-] equals 5 x 10⁻⁴ M. For every Ca(OH)₂ you produce 2 OH⁻<span>.
</span>
pOH = - log[ OH⁻]

pOH = - log [ <span>5 x 10⁻⁴ ]

pOH = 3.30

pH + pOH = 14

pH + 3.30 = 14

pH = 14 - 3.30

pH = 10.7

hope this helps!</span>
5 0
3 years ago
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