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SCORPION-xisa [38]
3 years ago
12

¿Todos los solutos se disuelven en cualquier solvente?

Chemistry
1 answer:
Katen [24]3 years ago
6 0

Answer:

No

Explanation: No. Todos los solutos tienen una solubilidad diferente, lo que significa que todos tienen una cantidad única de gramos que se disolverían en el mismo solvente. una solución que ha disuelto todo el soluto que puede contener a una temperatura determinada.

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) PABA refers to para-aminobenzoic acid which is used in some sunscreen formulations. If a 0.055 M solution of PABA has a pH of
AleksandrR [38]

Answer: K_a of PABA is 0.000022

Explanation:

NH_2C_6H_5COOH\rightarrow H^++NH_2C_6H_5COO^-

  cM              0             0

c-c\alpha        c\alpha          c\alpha

So dissociation constant will be:

K_a=\frac{(c\alpha)^{2}}{c-c\alpha}

Give c= 0.055 M and \alpha = ?

K_a=?

pH=-log[H^+]

2.96=-log[H^+]

[H^+]=1.09\times 10^{-3}

[H^+]=c\times \alpha

1.09\times 10^{-3}=0.055\times \alpha

\alpha=0.02

Putting in the values we get:

K_a=\frac{(0.055\times 0.02)^2}{(0.055-0.055\times 0.02)}

K_a=0.000022

Thus K_a of PABA is 0.000022

5 0
3 years ago
Show the calculation of the molar mass (molecular weight) of a solute if a solution of 5.8 grams of the solute in 100 grams of w
Leni [432]

Answer : The molar mass of solute is, 89.9 g/mol

Explanation : Given,

Mass of solute = 5.8 g

Mass of solvent (water) = 100 g

Formula used :  

\Delta T_f=K_f\times m\\\\T_f^o-T_f=T_f\times\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Mass of water}}

where,

\Delta T_f = change in freezing point

T_f^o = temperature of pure solvent (water) = 0^oC

T_f = temperature of solution = 1.20^oC

K_f = freezing point constant of water = 1.86^oC/m

m = molality

Now put all the given values in this formula, we get

(0^oC)-(1.20^oC)=1.86^oC/m\times \frac{5.8g\times 1000}{\text{Molar mass of solute}\times 100g}

\text{Molar mass of solute}=89.9g/mol

Therefore, the molar mass of solute is, 89.9 g/mol

5 0
3 years ago
Methane and water have different chemical properties because
jasenka [17]

Answer:

a

Explanation:

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3 0
3 years ago
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Select the correct answer.
vaieri [72.5K]

Answer:

b

Explanation:

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6 0
3 years ago
How many grams of oxygen can be produced from the decomposition of 100. g of kclo3?
aivan3 [116]
<span>100 g of KClO3 @ 122.55 g/mol = 0.816 moles of KClO3
   by the reaction
 2 KClO3 --> 2 KCl & 3 O2

   0.816 moles of KClO3 @ 3 moles O2 / 2 moles KClO3 = 1.224 moles of O2 can be made using molar mass
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6 0
3 years ago
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