(a)
Interpretation:To determine the concentration of H2CO3.
Concept Introduction:
Formula to calculate concentration:
(b)
Interpretation:To determine the concentration of HCO3-.
Concept Introduction:
Formula to calculate concentration:
(c)
Interpretation:To determine the concentration of hydronium ions, H3O+.
Concept Introduction :
Equilibrium constant may be defined as the ratio of product of concentration of products with the product of concentration of reactants and each concentration term has raised to the power equals to their respective
Mathematically,
Concentration of solid components is always taken as unity.
(d)
Interpretation: To determine the pH of given buffer solution.
Concept Introduction :
Relation between pH and hydronium concentration:
(e)
Interpretation: To write the balanced chemical equation which shows the neutralisation of added acid to given buffer solution.
Concept Introduction :
Buffer solution = It is a type of solution which can resist its pH when small amount of acid/base is added to it.
(f)
Interpretation: To write the balanced chemical equation which shows the neutralisation of added base to given buffer solution.
Concept Introduction :
Buffer solution = It is a type of solution which can resist its pH when small amount of acid/base is added to it.
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Basic Chemistry
- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardA buffer is made with sodium acetate (CH3COONa) andacetic acid (CH3COOH); the Ka for acetic acid is 1.80 x 10-5.The pH of the buffer is 3.98. What is the ratio of the equilibriumconcentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informationis given to answer this question.arrow_forwardMethanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENTarrow_forward
- Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. H₂S (aq) + KOH(aq) → 2- 3C₂² 1 2 + (s) S 3 K Reset 4 (1) 5 6 LO O 7 (g) ㅈ H 8 9 11 (aq) Submit X 0 • x H₂Oarrow_forwardWhat is the pH of a solution made by adding 0.65 m of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (K, = 1.8 x 105) %3D CH3CO2H (aq) + H2O (1) CH3CO2° (aq) + H3O* (aq) 4.74 O 5.08 04.40 8.92arrow_forwardOpen bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water. The dissolution of carbon dioxide produces carbonic acid (H2CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO2 (g) + H2O (l) H2CO3 (aq) H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq) The equilibrium between carbonic acid (H2CO3) and bicarbonate (HCO3-) is influenced by the presence of dissolved metals from the bedrock underlying a body of water. Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal. The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure). Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic acid/bicarbonate equilibrium?arrow_forward
- Using the following chemical equations, determine how the equilibrium will be affected if the pH is lowered? CO2(g) + H2O(l) ⟷⟷ H2CO3(aq) H2CO3(aq) ⟷⟷ H+1(aq) + HCO3-1(aq) There will be no effect on the equilibrium. More CO2(g) and more HCO3-1(aq) will be produced. Less CO2(g) will be produced and the HCO3-1(aq) concentration will increase. More CO2(g) will be produced. Less CO2(g) will be produced and the HCO3-1(aq) concentration will decrease.arrow_forward8 mL milk sample was titrated with 0.2 N NaOH by spending 3.2 mL. Calculate the% total acidity in milk in terms of lactic acid. (mEq: 0.09 (milli-equivalent gram of lactic acid found in milk). Convert the% total acidity in terms of lactic acid to total acidity in terms of citric acid. (1 lactic acid = 0.711 citric acid)arrow_forward7:30 1 y gmail x H Folde x A FINAL X E Prese x Prese x E PRESE X * Ceno x Y short x RI Anno x w weba x y chem x à app.101edu.co Time's Up! Write the acidic equilibrium equation for CH.NH:. 1 3 4 5 6 8 9 Os + (s) (1) (g) (ag) HO OH H:O H Reset • x H:O Delete (0) 7°C Mostly doudy a O od0 ENG P Type here to searcharrow_forward
- The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forwardA chemist has synthesized a monoprotic weak acid and wants to determine its pKa value. To do so, they dissolved 2.00 mmol of the solid acid in 100.0 mL of water and then titrated the resulting solution with 0.0500 M NaOH. After20.0 mL of added NaOH, the pH of the solution was 6.00. What is the pKa of the acid?(a) 5.85 (b) 7.02 (c) 9.90 (d) 6.00arrow_forwardConsider the following acid-base reaction: H3O+ + HPO42 H₂PO4 + H₂O Identify the Bronsted-Lowry base. OH₂O ⒸHPO4 ²- OH₂PO4 OH3O+ What is the concentration (in Molarity) of a Sulfuric Acid (H₂SO4) solution if a 15.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization? H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O (balanced) 0.012 M 0.025 M 0.836 M 0.270 Marrow_forward
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