3. Consider the distribution diagram for inorganic C in water. Answer the followingquestions.1.00.8CO₂ (H2CO3)Proportion of total inorganic C0.2i2900.4900.60.0HCO33456789101112PHCarbon dioxide dissolves in water according to the equilibriumCO2(g) + H2O(1) D H2CO3(aq).a. The average pH of surface ocean water is 8.14. In what form(s) (carbonic acid,bicarbonate ion, or carbonate ion) does most dissolved CO2 occur in oceanwater?

This distribution diagram shows how the different forms of inorganic carbon in water change with pH.…

Answered: 3. Consider the distribution diagram…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%
Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
11. (ii) A student was given 400 cm of aqueous ammonia solution, NH,(ag), The student was asked to determine how many moles of NH, had been dissolved to prepare the solution. The student titrated 25.0cm of NH.(ag) and found that it reacted exactiy with 32.5cm3 of 0.100 mol dm sulturic acid. The equation for this reaction is shown below. 2NH,(aq) + H,SO,(aq) → (NH)SO,(aq) Calculate the amount, in moles, of NH, in the original 400 cm3 solution. mol answer =
Gg.170.
- Calculate the concerntration of NaOH in the solution provided.
To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.
A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH21COOH21CH2COOH22, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.
3. Analysis of a mixture consisting of NaOH + Na2CO3 + inert matter gives the following data: 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample.
1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.
A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
Caculate the volume (mL) of 1.0 M potassium carbonate (K₂CO₃) needed to prepare 5.0g of the COPPER pigment. This is where the balanced chemical equation come in. You should be able to relate the moles of pigment to the moles of K₂CO₃, and from that calculate the volume of 1.0 M K₂CO₃ solution needed. Please report your value as XX.X mL (one deicmal point and no units).
6. (a) Aspirin is a weak acid with a pKa of 3.6 and MW 180 g/mol. The saturation solubility (S) of aspirin in water is 3.3 g /L and a saturated solution has pH equal to your answer to question 4(b) above. What is the solubility of the unionised form (So) of aspirin at this pH using units of mol/L and g/L. (b) Use the So value (just obtained) to calculate the saturation solubility (S) of aspirin in water at pH 6.6 using units of mol/L and g/L. (c) If you modified the aspirin suspension APF12 formula by replacing the purified water with pH 6.6 buffer, would the product be a suspension or solution?

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