The student titrated 10 ml of standered 0.15 M HCl with his sodium hydroxide solution. When the titration reached the equivalenc
1 answer:
Answer:
0.15 M
Explanation:
Step 1: Write the neutralization reaction
NaOH + HCl ⇒ NaCl + H₂O
Step 2: Calculate the moles of HCl that reacted
10 mL of 0.15 M HCl was used. The moles of HCl that reacted are:
Step 3: Calculate the moles of NaOH that reacted
The molar ratio of NaOH to HCl is 1:1. Then, the moles of NaOH that reacted are 1.5 × 10⁻³ moles.
Step 4: Calculate the concentration of NaOH
1.5 × 10⁻³ moles of NaOH are in 10.3 mL of solution. The molarity of NaOH is:
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Answer:
<em>»</em><em> </em><em>λ </em><em>=</em><em> </em><em>0</em><em>.</em><em>0</em><em>2</em><em>m</em>
Explanation:
Given :
Velocity of the wave {v}= 12 m/s
Frequency {f} = 600 Hz
Apply Wavelength formula :
•
→ λ =
→ λ =
→ λ = 0.02m
The pink color in the solution fades. Some of the colored indicator ion converts to the colorless indicator molecule.
<h3>Explanation</h3>What's the initial color of the solution?
is a salt soluble in water.
dissociates into ions completely when dissolved.
.
The first test tube used to contain .
is a weak base that dissociates partially in water.
.
There's also an equilibrium between and
ions.
.
ions from
will shift the equilibrium between
and
to the right and reduce the amount of
in the solution.
The indicator equilibrium will shift to the right to produce more ions along with the colored indicator ions. The solution will show a pink color.
What's the color of the solution after adding NH₄Cl?
Adding will add to the concentration of
ions in the solution. Some of the
ions will combine with
ions to produce
.
The equilibrium between and
ions will shift to the left to produce more of both ions.
The indicator equilibrium will shift to the left as the concentration of increases. There will be less colored ions and more colorless molecules in the test tube. The pink color will fade.