1.93•100^18 shshshshshshs

In a titration of 0.35 M HCl and 0.35 M NaOH, how much NaOH should be added to 45.0 ml of HCl to completely neutralize the acid?

Bezzdna [24]

It would be the same amount. So, 45 ml of NaOH is required to be added to the 45 ml of HCI to neutralize the acid fully. Here is a brief calculation:

Firstly, here is your formula: M(HCI) x V(HCI) = M(NaOh) x V(NaOH)
With the values put in: 0.35 x 45 = 0.35 x V(NaOH)
= 45 ml.
There is 45 ml of V(NaOH)

Let me know if you need anything else. :)

- Dotz

6 0

3 years ago

water is considered as a compound of hydrogen and oxygen and not a mixture of hydrogen and oxygen and comment on it

HACTEHA [7]

Wat is considered a compound of hydrogen and oxygen and not a mixture because hydrogen and oxygen have gone through a chemical process to form the compound h2O. A mixture can generally be easily separated whereas a compound must undergo another chemical process to separate its elements. Therefore to separate oxygen and hydrogen from water a chemical process is necessary.

4 0

4 years ago

For the reaction N2+3H2⇌2NH3, the metals Fe and Mo used as catalyst. which of the following is NOT a reason that catalysts have

Lubov Fominskaja [6]

D. Catalysts get used up in the formation of the product.

Catalysts are never used up in a reaction.

7 0

3 years ago

Calculate the amount of heat needed to boil 120.g of acetic acid (HCH3CO2), beginning from a temperature of 16.7°C.

evablogger [386]

Answer:

The total amount of heat needed = 72.2116 kJ

Explanation:

Given that ;

the mass of acetic acid = 120.0 g

The initial temperature $T_1$ = 16.7 °C = (16.7 + 273.15 ) K = 298.85 K

The standard molar mass of acetic acid = 60.052 g/mol

Thus ; we can determine the number of moles of acetic acid;

number of moles of acetic acid = mass of acetic acid/ molar mass of acetic acid

number of moles of acetic acid = 120.0 g/ 60.052 g/mol

number of moles of acetic acid = 1.998 moles

For acetic acid:

The standard boiling point $T_2$ = 118.1 °C = ( 118.1 + 273.15 ) K = 391.25 K

The enthalpy of vaporization of acetic acid $\Delta H_{vap}$ = 23.7 kJ/mol

The heat capacity of acetic acid c = 2.043 J/g.K

The change in temperature Δ T = $T_2 - T_1$

Δ T = (391.25 - 289.85)K

Δ T = 101.4 K

The amount of heat needed to bring the liquid acetic acid at 16.7°C to its boiling point is ;

q = mcΔT

From our values above;

q = 120 g × 2.043 J/g.K × 101.4 K

q = 24859.2 J

q = 24859 /1000 kJ

q = 24.859 kJ

we have earlier calculated our number of moles o f acetic acid to be 1.998 moles;

Thus;

The needed amount of heat = $\Delta_{vap} *numbers \ of \ moles$

The needed amount of heat = $23.7 \ kJ/mol * 1.998 \ moles$

The needed amount of heat = 47.3526 kJ

Hence;

The total amount of heat needed = 24.859 kJ + 47.3526 kJ

The total amount of heat needed = 72.2116 kJ

4 0

3 years ago

What is the mass of 20.0 L of sulfur dioxide (SO2) at STP?

larisa86 [58]

Answer:

Mass = 57.05 g

Explanation:

Given data:

Volume of SO₂ = 20.0 L

Temperature = standard = 273 K

Pressure = standard = 1 atm

Mass of SO₂ = ?

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K

T = temperature in kelvin

n = PV/RT

n = 1 atm × 20.0 L / 0.0821 atm.L/ mol.K× 273 k

n = 20.0 / 22.41/mol

n = 0.89 mol

Mass of SO₂:

Mass = number of moles × molar mass

Mass = 0.89 mol × 64.1 g/mol

Mass = 57.05 g

6 0

3 years ago