Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.170 M HClO(aq) with 0.170 M KOH(aq). The ionization constant for HClO can be found here.

In: Chemistry

At constant volume, the heat of combustion of a particular compound is –3680.0 kJ/mol. When 1.029 g of this compound (molar mass = 150.46 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 4.773 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

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Why is kcat not necessarily the best way to evaluate or compare the activities of two enzymes? What “adjustment” can be made to make the term more useful and why? A) Define the rate constants k1, k2 and k-1. Given k1 of 2x10^-8/M s, k2 of 5x10^3/s, and k-1 of 1x10^3/s, what is KD? what is KM? B) Which substrate is preferred: R, for which enzyme X has a KM of 2mM? OR Q, for which X has a KM is 7mM? Explain. If k2 for Q is 2x10^4/s and for R is 4x10^5/s, which substrate yields the best catalytic efficiency? Explain.

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3)Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250 M nitric acid. What is the final concentration of OH- ions in the solution after the reaction has gone to completion. Assume that there is no volume change when adding the grams of NaOH.

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100 mL of buffer solution that is 0.15M HA (K_{a}=
6.8x10^{-5}) and 0.20M NaA is mixed with 34.8mL of 0.35M
NaOH. What is the pH of the resulting solution?

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Consider the titration of 100.0 mL of 0.42 M H_{3}A by
0.42 M KOH for the next three questions. The triprotic acid has
K_{a1} = 1.0 x 10^{-4}, K_{a2} = 1.0 x
10^{-7}, and an unknown value for K_{a3}. All
answers to 3 significant digits.

1) Calculate the pH after 100.0 mL of KOH has been added.

pH =

2) Calculate the pH after 150.0 mL of KOH has been added.

pH =

3) The pH of the solution after 200.0 mL of KOH has been added
is 9.00. Determine the value of K_{a3} for this triprotic
acid. Use scientific notation to enter this answer, e.g., 1.0 x
10^{-3} = 1.0E-3.

Ka_{3} =

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Consider a solution that is 2.1×10^{?2} M in Fe2+and
1.8×10^{?2} M in Mg2+.

I know that the Fe2+ was the first to precipitate and that the minimum concentration of K2CO3 is

1.5×10 |
M |

What I need to know is **What is the
remaining concentration of the cation that precipitates first, when
the other cation just begins to precipitate?**

In: Chemistry

MnO2 (s) + 2 CO (g) → Mn (s) + 2 CO2 (g)

5. Calculate ΔG at 298K if MnO2 = 0.150 mol, Mn = 0.850 mol, CO = 0.250 M and CO2 = 0.500 M in a 1.25 L flask.

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This question has already been answered, but there was not as much detail as i needed to understand what exactly to do and i need to understand it quick... could you please walk me through how to do this, but specifically A and B please plug in all numbers and state where they came from , thank you so much!

Calculate the potential in the following cell

Pb|Pb2+(1.00M)|| Ag+(1.00M) |Ag

a. right at the beginning when you start using this voltaic cell,

b. when 50% of the Ag+ ions have been consumed,

c. when 99% of the Ag+ ions have been consumed, and

d. when 99.99% of the Ag+ ions have been consumed. Keep in mind that both, the Pb2+ and the Ag+ concentrations are changing.

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The Henry's law constant (k_{h}) for Ar in water at 20°C
is 0.0015 mol/(L atm). How many grams of gas will dissolve in 2.78
L of H_{2}O in contact with pure Ar at 1.6 atm?

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describe the actuve location (S) of hemoglobin and myoglobin.
How does the former function to transport 0_{2} from the
lungs to the cells where it is used?

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What is the silver ion concentration in a solution prepared by mixing 413 mL 0.356 M413 mL 0.356 M silver nitrate with 453 mL 0.438 M453 mL 0.438 M sodium phosphate? The KspKsp of silver phosphate is 2.8×10−18.

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The reaction A → B + C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time.

Time, h |
[A], M |

0.5 | 5.00 x 10^{-2} |

1 | 4.51 x 10^{-2} |

2 | 4.06 x 10^{-2} |

3 | 3.30 x 10^{-2} |

4 | 2.18 x 10^{-2} |

5 | 1.77 x 10^{-2} |

6 | 1.44 x 10^{-2} |

**(a)** What is the **average rate**
of reaction between 0.5 and 2 h? Report the units as well as the
numbers.

**(b)** Plot the data above, showing the
concentration of A as a function of the time. From your graph,
determine the **instantaneous rate** of reaction at 4
h. Report the units as well as the numbers.

**(c)** Plot ln [A] versus time. Estimate the rate
constant for this first-order reaction from your graph. Report the
units as well as the numbers.

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A student is examining a bacterium under the microscope. The E. coli bacterial cell has a mass of m = 1.80 fg (where a femtogram, fg, is 10−15g) and is swimming at a velocity of v = 2.00 μm/s , with an uncertainty in the velocity of 5.00 % . E. coli bacterial cells are around 1 μm ( 10−6 m) in length. The student is supposed to observe the bacterium and make a drawing. However, the student, having just learned about the Heisenberg uncertainty principle in physics class, complains that she cannot make the drawing. She claims that the uncertainty of the bacterium's position is greater than the microscope's viewing field, and the bacterium is thus impossible to locate. Part A What is the uncertainty of the position of the bacterium

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Answer the following questions based on HSAB theory. If using Fajans Rules, give the rule number and explain why it applies.

1. Explain why aluminum perchlorate is less soluble than aluminum cyanide. This is unusual since perchorates tend to be very soluble.

2. Explain why the Ksp for FeBr2 is 4.1 x 10–4 and the Ksp for FeF2 is 3.2 x 19–7.

3. Explain why the Ksp for Fe(OH)3 is 1.2 x 10–36 and the Ksp for Fe(OH)2 is 7.8 x 10–16.

4. Explain why VS is more soluble than NiS.

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