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1.Above you will find a graph of a monoprotic weak acid titration. In this titration a 0.5053 g sample ...

e of a weak acid in 32.9 mL of water is titrated with 0.0755 M Ca(OH)2. Calculate the molarity of the weak acid being utilized in the titration above. (do not provide units and follow significant figure rules).

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in water and dissociates, C2O4
2- is a polyatomic ion.
a. Calculate the molar solubility of sodium oxalate.
b. Calculate the Ksp for sodium oxalate.
c. Calculate the total ion concentration for a solution where 1.33 g of sodium
oxalate is added to 20.0 mL of water.

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3. 23.0 mL of water are put in a graduated cylinder. The cylinder with the water in it has a mass ...

144.7 g. The dry, empty cylinder has a mass of 121.2 g

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rite only the answer to two decimal digits

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5.A cube of iron with edges 4.0 cm long is initially at 750°C. It is then dropped into 250 mL ...

r at 20°C.
[6 points] Ignoring any heat transfer to the container and the environment, calculate the percentage of water that is boiled away.
[2 points] Would accounting for heat transfer to the container and the environment make your answer to part (a) larger or smaller? Explain.

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6.(a) A 20.0 L container at 303 K holds a mixture of two gases with a total pressure of 5.00 ...

here are 2.00 mol of Gas A in the mixture, how many moles of Gas B are present? (R = 0.0821 L • atm/(K • mol))
(b) The gas in a 250. mL piston experiences a change in pressure from 1.00 atm to 2.80 atm. What is the new volume (in mL) assuming the moles of gas and temperature are held constant?
(c) Small quantities of Oxygen can be produced by the decomposition of mercury(II) oxide as shown below. Typically, the oxygen gas is bubbled through water for collection and becomes saturated with water vapor. Atomic weight of HgO = 216.6 amu, Atomic weight of Oxygen = 32.00 amu)
2 HgO(s) → 2 Hg(ℓ) + O₂(g)
(i) Assuming that 3.05 grams of HgO was used in this reaction, determine the number of moles of oxygen gas formed.(According to the above chemical equation)
(ii) Assuming 310. 0 mL of Oxygen gas was collected at at 29°C, calculate the pressure of the Oxygen gas that was collected. (R = 0.0821 L • atm/(K • mol)
(iii) If the vapor pressure of water at this temperature equals to 0.042 atm, calculate the pressure reading of this experiment.

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you dissolve in water to make a 0.2 M calcium chloride solution with 200 mL final volume?

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r to produce a final concentration of 4%?

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lar mass -KMnO4 = 158 g/mol) used in titration of 100 mL raw-water sample diluted 1:20 was 9,2 mL. Calculate the orientative amount of Fe(III)-sulfate coagulant needed to be added to 600mL of water sample in a coagulation-flocculation experiment.

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10.A volume of 125 mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ...

∘C is placed in the water. If the final temperature of the system is 21.40 ∘C , what is the mass of the steel bar?
specific heat of water = 4.18 J/(g⋅∘C)
specific heat of steel = 0.452 J/(g⋅∘C)

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11.5 (5 points) There is H3PO4 available in stock solution that has an assay of 77% and a density ...

cific gravity) of 1.24. What is the molarity of this solution?
Using this solution how would 1 L of 2N solution be made.
6 (5 points) H3BO3 is needed to neutralize 20 ML of a 2N solution of NaOH. How much of the acid should I put in 40 ML of the water to exactly neutralize this solution?
7 (6 points) Describe how to make the solutions below :
20% w/v Salt in water.
20% v/v alcohol in water
20% w/w NaCl in water.
8 (three points) I have 0.6 g/dl solution of NaOH. What is M? Whan is N?
9 (six points) There are 3000mL of 3M NaOH. How much of the following do I need to neutralize? (watch your M’s and N’s
a) 3M H3PO4
b) 2M H2SO4
c) 1M HCL
10 (20 points) The following solutions of NaOH are mixed together 20ML of 3N, 40mL of 2N, 60mL of 1N, 80 mL of 4N, and 100mL of 5N.
a) What is the volume and normality of the final solution?
b) How much 4M sulfuric acid would I need to neutralize?
c) How much stock solution of sulfuric acid with an assay of 77% and a specific gravity of 1.14 would I need?
d) How many grams of HCl would I have to put in a 300mL solution of HCl in water to neutralize?
11 (3 points) How much 5N solution can I make with 98 grams of H3PO4 ?
12 (5 points) How much 5N solution of H3AsO4 can I make with 57 mL of stock solution that is 84% assay and 1.14 specific gravity?
13 (5 points) If we have a 4N solution of HCl that has 0.03645g of HCl in the solution, how many microliters of solution do we have?
14 (10 points) If we have 66mL of a solution of concentrated NaOH that has an assay of 88% and a specific gravity of 1.24, how much 3N H3AsO4 can be neutralized?
15 (ten points) If I have 17 mL of a 20% w/v solution of NaOH and I want to neutralize with H2SO4 that is available in a 4% w/v solution, how much of this solution will be required.
16 (ten points)
a) I have an 12mL of Ba(Cl)2 that is 78% assay that contains 8 grams of Ba(Cl)2. What is the specific gravity?
b) How many Moles of Ba(Cl)2 are there?
c) If I have 80 grams of NaOH in a liter of solution that is of an unknown specific gravity, can I calculate molarity and what is it?
d) What is the difference between molarity and normality?
e) I have 77 ml of 77% salt in water. How much 11% can I make?

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12.I was wondering if you could help me step up my chem problems, i'm not sure how to begin ...

estion 1: Draven collected a 1ml sample from a local river. Draven added 99 ml of water to the sample. Draven then took 5 ml of the diluted sample, and determined the 5 ml sample to contained 10 mg of sodium chloride. what is the concentration of sodium chloride in the river?
question 2: how many grams of H2 could be produced when 13 g of H202 decompose?
question 3: how many molecules of carbon dioxide could be produced when 25 ml of a 0.8 M ethanol, c2h60, combusts with 5.18X10^23 molecules of oxygen? the unbalanced equation for the combustion of ethanol is given below:
2ch6O+302-> c02+h20

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, What would be the predicted concentration of HCB due to bioconcentration in the fat of fish that swim in water containing 0.00006 ppm of the chemical?
2. The fat content of breast milk averages a little over 4.0 g per 100 ml. Calculate the mass of DDE that would have been ingested by a typical breast-fed infant in 1972 consuming 300 ml of breast milk per feeding, if the milk contained about 500 ppb of DDE in its fat content.
3. The PCB concentration in Lake Michigan is declining according to a first-order rate law having a rate constant of 0.078 year-1. If the PCB concentration in the lake averaged 0.057 ppt (parts per trillion) in 1994, what was the concentration in 2004? In what year will the concentration fall to 0.005 ppt.

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1.AU MAT 120 Systems of Linear Equations and Inequalities Discussion

mathematicsalgebra Physics