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Alja [10]
3 years ago
14

What are 5 questions that have the answer scicne safety

Chemistry
1 answer:
lisabon 2012 [21]3 years ago
8 0

Answer:

Explanation:

What is the question?

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A 400.0 ml sample of 0.10 mba(oh)2 is titrated with 0.10 mhbr. determine the ph of the solution before the addition of any hbr.
Leno4ka [110]
Ba(OH)2 is an basic solution. It has more OH- ions than H+ ions. pOH should be calculated to find out its pH
The reaction is
Ba(OH)2 ⇒ Ba2+ (aq) + 2 OH-(aq)
One mole barium hydroxide releases 2 moles hydroxide ions.

Use that ratio to calculate molarity (M) of OH- ions [OH-]. The ratio is 1:2. 
0.10 M Ba(OH)2 release 2*0.10 M= 0.02 M OH- ions
[OH-]= 0.02
pOH= - log [OH-] = - log 0.02 = 1.7
Thats not the answer! We found pOH of the solution before titration.
pH and pOH relationship is shown by formula of pH+pOH= 14 
pH= 14-pOH
pH= 14-1.7= 12.3

7 0
4 years ago
Read 2 more answers
What will be the ph of a buffer solution with an acid (pka6. 1) that is exactly half as concentrated as its conjugate base?
anygoal [31]

The pH of a buffer solution with acid that (PKA 6. 1) is exactly half as concentrated as its conjugate base is 6.4.

<h3>What is a buffer solution?</h3>

A buffer solution is a solution that has a maintained pH, not basic or not acidic. Its pH changes when acid or base is added to the solution.

We had to figure out the acid's concentration, which is exactly half that of its potential base.

We know that pH = pH_log

We have less than 6.1 pH so this is a conjugated base.

This will equal to 6.1 + log2 = 6.4

Thus, the pH of a buffer solution with acid is 6.4.

To learn more about buffer solutions, refer to the below link:

brainly.com/question/13169083

#SPJ4

7 0
2 years ago
In an ionic bond:
xz_007 [3.2K]
The answer I'm pretty sure is a because it can't be d because ionic binding the electrons are affected and it can't be c because that's covalent bonding and it can't be b because they don't swap electrons.
3 0
3 years ago
Read 2 more answers
The elementary reaction 2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2, and O2
jenyasd209 [6]

Answer:

1.742\times 10^{-5} is the value of the equilibrium constant at this temperature.

Explanation:

2H_2O\rightleftharpoons 2H_2+O_2

We are given:

Partial pressure of H_2O=p^o_{H_2O}=0.0750 atm

Partial pressure of H_2=p^o_{H_2}=0.00700 atm

Partial pressure of O_2=p^o_{O_2}=0.00200 atm

The expression of K_p for the given chemical equation is:

K_p=\frac{p^o_{H_2}^2\times p^o_{O_2}}{p^o_{H_2O}^2}

Putting values in above equation, we get:

K_p=\frac{(0.00700 atm)^2\times 0.00200 atm}{(0.0750 atm)^2}\\\\K_p=1.742\times 10^{-5}

1.742\times 10^{-5} is the value of the equilibrium constant at this temperature.

3 0
4 years ago
A_______ will flow only sideways and down
bezimeni [28]

Answer:

A liquid will flow only sideways and down

Explanation:

   

5 0
3 years ago
Read 2 more answers
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