Answer:
[Na₂CO₃] = 0.094M
Explanation:
Based on the reaction:
HCO₃⁻(aq) + H₂O(l) ↔ CO₃²⁻(aq) + H₃O⁺(aq)
It is possible to find pH using Henderson-Hasselbalch formula:
pH = pka + log₁₀ [A⁻] / [HA]
Where [A⁻] is concentration of conjugate base, [CO₃²⁻] = [Na₂CO₃] and [HA] is concentration of weak acid, [NaHCO₃] = 0.20M.
pH is desire pH and pKa (<em>10.00</em>) is -log pka = -log 4.7x10⁻¹¹ = <em>10.33</em>
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Replacing these values:
10.00 = 10.33 + log₁₀ [Na₂CO₃] / [0.20]
<em> [Na₂CO₃] = 0.094M</em>
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Answer:
Some human activities that cause damage (either directly or indirectly) to the environment on a global scale include population growth, overconsumption, overexploitation, pollution, and deforestation, to name but a few.
Explanation:
Hope this helped!!!
Answer:
5.59 %
Explanation:
From the question given above, the following data were obtained:
Observed value of density = 2.85 g/cm³
True value of density = 2.699 g/cm³
Percentage error =.?
The percentage error of the student can be obtained as follow:
Percentage error = |Observed value – True value|/True value × 100
Percentage error = |2.85 – 2.699|/2.699
Percentage error = 0.151/2.699 × 100
Percentage error = 5.59 %
Therefore, the percentage error of the student is 5.59 %.
Answer:
Definition:
Titration is a quantitative technique where solution of known concentration is used to determine the concentration of unkown solution.
Explanation:
Titration is a quantitative technique where solution of known concentration is used to determine the concentration of unkown solution. it is also called titrimetry or volumetric analysis.
Titrant:
The known solution is called titrant. Titrant is prepared from the standard solution of known concentration and volume. It is added from the burette to the analyte.
Analyte:
The substance whose concentration or quantity is to be determine is called analyte. Titrant is carefully added to the analyte to carry out the reaction untill the end point is reached.
Usually the indicator are used to signal the end point.
End point:
It is also called equivalence point. it is the point where indicator shows that the amount of titrant needed to complete the reaction is added to the solution. it is indicated by colour changes during the reaction.
Procedure:
1. The burette is filled with titrant.
2. The flask is filled with the analyte.
3. One drop of indicator is added to the analyte before satrting the titration.
4. Now the titrant is added slowly into the analyte, drop wise until the indicator show the colour which indicate the end point.
5. After the end point is reached, note the burette reading.
6. At the end of titration final calculations can be done.
Types of titration:
Acid-Base titration
Redox titration