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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24. When the acidity provided by the dissolved carbon dioxide and the basicity provided by the solid CaCO3 are both considered, the single reaction that best represents what happens when solid CaCO3 dissolves in water in contact with atmospheric carbon dioxide at a partial pressure Pis the following: CaCO3(s) + CO2 (g) + H2O = Ca2+(aq) + 2HCO3 (aq) a. Using the approach of adding reactions, show that the equilibrium constant for the above reaction is given by: K' = KspkHKai/Ka2 where the equilibrium constants have been defined in the earlier problems 1-3; calculate a numerical value for K' from the numerical values at 25° C that have been given. b. Use the value calculated for K' to determine the concentration of Ca2+(ag) and HCO3 (ag) in water that is in equilibrium with solid CaCO3 and water that is exposed to the nominal partial pressure of atmospheric carbon dioxide, 0.000405 atm. c. Compare the solubility calculated by this approximation with the values found for the water samples…
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%
Gg.170.
- Calculate the concerntration of NaOH in the solution provided.
15). If Ca(NO3) (aq) is slowly added to solution containing CO32– and SO42– what compound would precipitate out first given the solubility products (Ksp (CaSO4) = 2.4 x 10–5 and Ksp (CaCO3) = 8.7 x 10–9)? CaCO3 would precipitate first because it is least soluble. CaSO4 would precipitate first because it is least soluble. CaCO3 would precipitate first because it is more soluble. CaSO4 would precipitate first because it is more soluble.
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 solution of Na,SO, in water is saturated at 50°C. When a saturated solution of Na,SO, is cooled, crystals of Na,SO4-10H2O separate from the solution Temperature, °C Solubility of Na,SO, g/100g water 49 50 46.7 10 9 If 1000 kg of this solution is cooled to 10°C, the percentage yield obtained is nearly а. 91 b. 90 с. 100 d. 80
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.
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.
TUOv to lls worla taum uo 1o9TIOoni bolam od lliw elimu iboo lut o 19 4. Given the Borax reaction below, what would be the solubility product (Ksp) of borax at 40 °C, if the solubility of borax is 0.8 mol L¯1 at 40 °C? Na,B4O5 (OH)4 · 8H,O(s) = 2Na+ (aq) + B405(OH) (aq) +8H,O(1) sr vol (A) gnsb vgotino brrbae ar bo CHO)gab xglerino bisbasie orb il S
КНР (ад) + NаОН (ад)- - NAKHP (aq) + H20 (1) Trial V; (mL) V; (mL) 33.87 45.73 2 A student masses out 1.019 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NAOH, as shown in the equation above. Calculate the molarity of the NaOH solution. RE FS F6 F7 FB F10
4. a) Calculate AG° for the following reaction, using the provided information. 2 C6H6(1) + 15 02(9) → 12 CO2(9) + 6 H20 (g) AG°;(CO2(9) = -394. 6 "/mol AG°(H20(9) = -228.4 (g) mol AG°,(H20u) = -237.2 k mol kJ AG°,(C,H6») = -121.7 K/ тol

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