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What is the difference between measured and accepted value? And how are these values used to determine the precision of these va

serg [7]

Measured values are verified and go under a series of experiments before being accepted as the norm. Accepted values are unanimously accepted values, seen as the norm by a qualified group of individuals (scientists or the people of the intellectual sphere).

7 0

3 years ago

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True or false : Color Changes are used to show reaction completion

Aleks [24]

Answer:

True

Explanation:

It means the reaction is occuring.

7 0

3 years ago

What kind of change took place when the magnesium was heated?

Dmitrij [34]

Answer:

You can see that it is an endothermic reaction or heat is being absorbed for the change from magnesium to magnesium oxide. So it is an endothermic reaction. So these are the four reasons why we can say that burning of magnesium ribbon in the air is considered a chemical change.

Explanation:

hope it help

6 0

3 years ago

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3.364 g of hydrated barium chloride of BaCL2.xH2O was dissolved in water and made up to a total volume of 250.0 mL. 10.00 mL of

atroni [7]

Given:

Mass of hydrated barium chloride = 3.364 g

Total volume of barium chloride V(total)= 250 ml

Volume taken for titration V = 10 ml

Volume of AgNO3 consumed = 46.92 ml

Concentration of AgNO3 = 0.0253 M

To determine:

The value of x i.e. the water of hydration in BaCl2

Explanation:

The net ionic equation is-

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Based on the reaction stoichiometry: Equal moles of Ag+ and Cl- combine to form AgCl

Moles of Ag+ consumed = moles of Cl- present

Moles of Ag+ = V(AgNO3) * M(AgNO3) = 0.04692 * 0.0253 = 0.00119moles

Moles of Cl- present = 0.00119 moles

Thus, 0.00119 moles of Cl- are present in 10 ml of the solution

Therefore, number of moles of Cl- in 250 ml would be-

= 0.00119 * 250 /10 = 0.02975 moles of cl-

Now:

2 moles of Cl- are present in 1 mole of BaCl2

Therefore, 0.02975 moles of Cl- correspond to- 0.02975 * 1/2 = 0.01488 moles of BaCl2

Molar mass of BaCl2 = 208.22 g/mol

Thus, mass of BaCl2 = 0.01488 moles * 208.22 g.mol-1 = 3.098 g

Mass of water of hydration = 3.364 - 3.098 = 0.266 g

# moles of water 'x' = .266/18 = 0.015 ≅ 1

Ans: Formula for hydrated barium chloride = BaCl2. 1H2O

7 0

4 years ago

Calculate the molarity of the NaCl solution when 43.8 g of NaCl is dissolved in 100 mL of water.

Ad libitum [116K]

Answer: The molarity of solution is 7.45 M

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

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

where,

n = moles of solute

$V_s$ = volume of solution in ml

moles of $NaCl$ = $\frac{\text {given mass}}{\text {Molar mass}}=\frac{43.8g}{58.5g/mol}=0.745mol$

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

$Molarity=\frac{0.745\times 1000}{100}$

$Molarity=7.45M$

Therefore, the molarity of solution is 7.45 M

7 0

3 years ago