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- Apatite, Ca5(PO4)3OH, is the mineral in teeth. On a chemical basis explain why drinking milk strengthens young children’s teeth. Sour milk contains lactic acid. Not removing sour milk from the teeth of young children can lead to tooth decay. Use chemical principles to explain why.5. If magnesium hydroxide were used instead of NaOH, how many moles would it take to combine with three moles of KHP? Explain.31. A sample of meat scrap weighing 2.000 g is digested with concentrated H2SO4 and a catalyat. The resulting solution is made alkaline with NaOH and the liberated ammonia distilled into a 50.0 mL of 0.6700 N H2SO4. The excess then requires 30.10 mL of 0.06520 N NaOH for neutralization. What is the percentage of nitrogen in the meat?
- The Solvay process for the manufacture of a sodium carbonate begins by passing ammonia and acrbon dioxide through a solution of sodium chloride to make sodium bicarbonate and ammonium chloride. The equation for this reaction is: H2O + NaCl + NH3 + CO2 -> NH4Cl + NaHCO3 In the next step, sodium bicarbonate is heated to give sodium carbonate and two gases, carbon dioxide and steam. 2NaHCO3 -> Na2CO3 + CO2 + H2O 1. What is the theoretical yield of sodium carbonate, expressed in grams, if 164 g of NaCl were used in the first reaction? 2. If 77.9 g of Na2CO3 was obtained, what was the percentage yield?Calculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is measured to be 1.49. Use this information to determine a value of Ka for chlorous acid. HCIO₂(aq) + H₂O(l)=CIO₂ (aq) + H₂O˚(aq) K₂ =1. State Le Chatelier’s Principle. If the equilibrium constant (K) ˃ 1, what will be the direction of the equilibrium position? [A/3]
- 1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.3. The pH of blood is buffered by a mixture of HCO3- (bicarbonate) and H2CO3 (carbonic acid).i. Write out an equation that shows a reaction of H+ with HCO3-iii. Recall that H2CO3 (aq) decomposes readily. Write a chemical equation to describe this decomposition. The pH of blood is buffered by a mixture of HCO3- (bicarbonate) and H2CO3 (carbonic acid). Write out an equation that shows a reaction of H+ with HCO-3. Recall that H2CO3 (aq) decomposes readily. Write a chemical equation to describe this decomposition. Consider your response to the last question and explain how bicarbonate and carbonic acid are generated by the dissolving of CO2 in water (Hint: The reaction for “ii” is reversible.)4. Write a dissociation equation for the following: a) CaCl b) Al-(SO.)x0).
- ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?1. A 1.2040 g sample containing sodium carbonate and inert material was dissolved in water and titrated to methyl orange end point, requiring 32.50 mL of 0.1020 M HCl. Calculate the %Na2CO4 in the sample. a. 93.36% b. 14.59% c. 12.75% d. 23.41%2. A 0.1510 g KHP (MW = 204.22 g/mol) sample required a volume of 57.04 mL of NaOH solution to reach a phenolphthalein end point. Calculate the molarity of NaOH titrant. a. 0.02593 M b. 0.006481 M c. 0.01296 M d. 0.01012 MRank the following solutions according to their acidity: solution one: pH=12 (least acidic,intermediate acidity, or most aciditic) Solution one: [h3O+]= 10-8 M (least acidic, intermediate acidity, or most aciditic) solution three: [OH-)= 10-10 M (Least acidic, intermediate acidity, or most aciditic)