All categories

3 years ago

If I added 50 mL of a 1.0 M HCIO2 solution to 50 mL of a 1.0 M NaOH

Chemistry

1 answer:

kozerog [31]3 years ago

3 0

Answer:

pH=7

Explanation:

0.05 L*1.0M= 0.05 mol HClO2 and 0.05 mol NaOH

HClO2 + NaOH ---> NaClO2 + H2O

0.05 mol 0.05 mol

As we can see acid and base react completely, solution will be neutral, so pH =7

You might be interested in

What is the oxidation state of cl in hclo4?

Irina-Kira [14]

There is 1 H atom: (1)(+1) = +1 The oxidation number of O is -2. There are 4 O atoms here: (4)(-2) = -8 So the oxidation state of Cl is +7.

NOTE: The maximum positive oxidation number for chlorine is +7, the same as its group number (VII).

3 0

3 years ago

Read 2 more answers

Using ethanol and sodium or potassium cyanide as the sources of the carbon atoms, along with any necessary inorganic reagents, s

11Alexandr11 [23.1K]

Answer:

Please see attachment

Explanation:

Please see attachment

3 0

3 years ago

What does resonance result in?

Tcecarenko [31]

louder sounds

Explanation:

Resonance results in louder sounds.

Resonance is a phenomenon that produces a large vibration as a result of smaller vibration that causes the resonating body to vibrate at its own natural frequency.

Resonance results in sound amplification and causes louder sounds. Increasing vibration results in the production of a louder sound.

Learn more:

Resonance in chemistry brainly.com/question/9422880

#learnwithBrainly

3 0

3 years ago

How much of a 10 M solution is needed to make 1 liter of all solution?

SashulF [63]

Answer:

b is the answer 1000ml

please mark me brainlist

4 0

3 years ago

Iron (III) oxide and hydrogen react to form iron and water, like this: Fe 03(s)+3H9)2Fe(s)+3HO) At a certain temperature, a chem

belka [17]

The question is incomplete, here is the complete question:

Iron (III) oxide and hydrogen react to form iron and water, like this:

$Fe_2O_3(s)+3H_2(g)\rightarrow 2Fe(s)+3H_2O(g)$

At a certain temperature, a chemist finds that a 8.9 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, Iron, and water at equilibrium has the following composition.

Compound Amount

Fe₂O₃ 3.95 g

H₂ 4.77 g

Fe 4.38 g

H₂O 2.00 g

Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to 2 significant digits.

Answer: The value of equilibrium constant for given equation is $1.0\times 10^{-4}$

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

For hydrogen gas:

Given mass of hydrogen gas = 4.77 g

Molar mass of hydrogen gas = 2 g/mol

Volume of the solution = 8.9 L

Putting values in above expression, we get:

$\text{Molarity of hydrogen gas}=\frac{4.77}{2\times 8.9}\\\\\text{Molarity of hydrogen gas}=0.268M$

For water:

Given mass of water = 2.00 g

Molar mass of water = 18 g/mol

Volume of the solution = 8.9 L

Putting values in above expression, we get:

$\text{Molarity of water}=\frac{2.00}{18\times 8.9}\\\\\text{Molarity of water}=0.0125M$

For the given chemical equation:

$Fe_2O_3(s)+3H_2(g)\rightarrow 2Fe(s)+3H_2O(g)$

The expression of equilibrium constant for above equation follows:

$K_{eq}=\frac{[H_2O]^3}{[H_2]^3}$

Concentration of pure solids and pure liquids are taken as 1 in equilibrium constant expression.

Putting values in above expression, we get:

$K_{c}=\frac{(0.0125)^3}{(0.268)^3}\\\\K_{c}=1.0\times 10^{-4}$

Hence, the value of equilibrium constant for given equation is $1.0\times 10^{-4}$

6 0

4 years ago