Concept explainers
Interpretation:
The pH of the solution, obtained by dissolving the product, of the given reaction, in water, at a temperature of
Concept introduction:
Equilibrium constant isdefined as the ratio of concentration of products to the concentration of reactants and is expressed as follows:
Molarity is defined as the number of moles of solute dissolved in one litre of solution and is expressed as follows:
Answer to Problem 101AP
Solution: pH is
Explanation of Solution
Given information: The white phosphorous burnt is
The volume of solution is
If the white phosphorus burns in excess of oxygen, the reaction is as follows:
The product formed
The moles formed by
Substitute the values in the above equation:
Thus, the moles of
Molarity of the phosphoric acid solution is calculated as follows:
Substitute
The equilibrium expression for a phosphoric acid solution is as follows:
The value of
The
Substitute
Rearrange the above equation:
This is a quadratic equation, by solving:
The pH of the solution is to be calculated as follows:
Here, the concentration of hydronium ions
The pH of the solution at
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Chapter 24 Solutions
Chemistry
- When carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)arrow_forwardThe reaction of calcium hydride, CaH2, with water can be characterized as a Lewis acid-base reaction: CaH2(s)+2H2O(l)Ca(OH)2(aq)+2H2(g) Identify the Lewis acid and the Lewis base among the reactants. The reaction is also an oxidation-reduction reaction. Identify the oxidizing agent, the reducing agent, and the changes in oxidation number that occur in the reaction.arrow_forwardThe formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why.arrow_forward
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- Explain how ammonia can function both as a Brønsted base and as a Lewis base.arrow_forwardConsider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10arrow_forwardCalculate the pH of a 0.10 M solution of sodium hypochlorite (NaClO; Ka 2.90 x 10$). Also, calculate the pH after diluting the solution by 10 times.arrow_forward
- 1. Calculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5. 2. Calculate the pH of a 0.055 M AlCl3 (aq) (aluminum chloride) solution. Ka for Al3+ is 1.2 × 10–5.arrow_forwardCalculate the pH for a 0.200 M KClO2 aqueous solution. (Ka for HClO2 is 1.1× × 10–2).arrow_forwardPhosphoric acid (H,PO4) is a polyprotic acid. Write balanced chemical equations for the sequence of reactions that phosphoric acid can undergo when it's dissolved in water.arrow_forward
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