Concept explainers
(a)
Interpretation:
The required volume ratio of the acid solution given in the question should be calculated.
Concept introduction:
When acid and base reacts, it forms salt and water which is called as neutralization. This reaction involves the combination of positively charged H and negatively charged OH ions to form water molecule. The neutralization of an acid and a base has pH value of 7.
In the above question a 10.0mole% aqueous sulfuric acid solution reacts with a 3.00molar caustic soda solution till they are neutralized at
The acid neutralizes reaction is shown below:
(b)
Interpretation:
The standard heats of formation for the three solutions involved and heat released when the reactants are at
Concept introduction:
When acid and base reacts, it forms salt and water which is called as neutralization. This reaction involves the combination of positively charged H and negatively charged OH ions to form water molecule. The neutralization of an acid and a base has pH value of 7.
The acid neutralizes reaction is shown below:
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Chapter 9 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?arrow_forwardAn artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forward
- Calculate the minimum concentration of NH3 needed to dissolve 2.00x 10 -3 mol of AgBr in 1.00 L solution. AgBr(s) → Ag' (aq) + Br (aq) Kgp = [Ag'][Br] = 5 x 1013 %3D Ag (aq) + 2NH3 (aq) → Ag(NH3)2* (aq) K; = 1.7 x 107 %3D O 1.03 M O 0.690 M O 0.686 M O 0.688 O 4.52 Marrow_forwarddium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide A student prepares a dilute solution of sodium hydroxide, NaOH(aq), starting with 6 M so- sodium hydroxide, NaOH(aq), calculate the molar concentration of the sodium hydroxide solution, NaOH(aq). (Remember that KHP is potassium hydrogen phthalate, KHC,H¸O, solution, NaOH(aq), to a phenolphthalein end point. If the titration required 21.84 mL of NOT potassium hydrogen phosphorus!) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphtha- lein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH(aq), calculate the molar concentration of acetic acid, HC,H,0,(aq), in the vinegar. Calculate the mass percent of acetic acid, HC,H¸0,(aq), in the vinegar using the molar con- centration for acetic acid, HC,H,0,(aq), determined in part b and assuming the density of the solution is 1.01 g/mL.arrow_forwardLimestone consists mainly of the mineral calcite, CaCO 3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO 2: CaCO 3(s) + 2 HCl → CaCl 2 + CO 2(g) + H 2O The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.arrow_forward
- Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO2: CaCO3(s, 100.087 g/mol) + 2 H+ → Ca2+ + CO2(g) + H2O The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.arrow_forwardA sodium hydroxide solution is standardized by titrating 0.8592 g of ordinary standard potassium hydrogen phthalate (204.22 g/mol) to a phenolphthalein end point, requiring 32.67 ml. What is the molarity of the NaOH solution? cO,K cO;K + NaOH + H,0 COH Pim yg plaarrow_forwardAssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO₂H, in enough water to make 5.00 x 10² mL of solution and then titrate the solution with 0.168 M NaOH. C6H5CO₂H(aq) + OH(aq) → C6H5CO₂ (aq) + H₂O(l) What are the concentrations of the following ions at the equivalence point? 0.0037 1.30e-8 Na+, H3O+, OH™ C6H5CO₂ X M Na+ ✓ MH 30+ X MOH™ 7.66e-7 0.0037 XM C6H5CO₂ What is the pH of the solution? 7.86arrow_forward
- The following two solutions are mixed together: 125.0 mL of 0.2798 MPb(C2H3O2)2(aq) and 275.0 of 0.1901 M KCl(aq)Pb(C2H3O2)2(aq) + 2 KCl(aq) → PbCl2(s) + 2 KC2H3O2(aq)Determine the final concentration of K+ and Pb2+ in solution. Assume the volumes areadditive.arrow_forwardA buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution.arrow_forwardA buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution. d) What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?arrow_forward
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