Determine the volume (in mL) of 0.411 M hydrochloric acid (HCl) that must be added to 448 mL of 0.914 M sodium butanoate (NaC3H7COO) to yield a pH of 5.48. Assume the 5% approximation is valid and report your answer to 3 significant figures. A table of pKa values can be found here. pKa=4.82

For the following reaction, 10.1 grams of propane (C3H8) are allowed to react with 20.6 grams of oxygen gas . propane (C3H8)(g) + oxygen(g) carbon dioxide(g) + water(g) What is the maximum amount of carbon dioxide that can be formed? _ grams

What is the FORMULA for the limiting reagent?

What amount of the excess reagent remains after the reaction is complete? _ grams

You have an unknown dye solution whose concentration seems to lie between 0.0006M stock solution and a 0.0004 stock solution. Therefore, you had planned to dilute the 0.0006M stock to create your calibration standards. However, you see that there is no 0.0006M stock left but there is plenty of they 0.0004M stock

a. How could you raise the concentration of some of the 0.0004M stock to make 75mL of a 0.0006M solution without adding any more dye? Be sure to show calculations and indicate that volume of 0.0004M required.

b. Please draw a molecular view picture illustrating the moles of dye remaining constant during this process

A 25.0 mL sample of a 0.3400 M solution of aqueous trimethylamine is titrated with a 0.4250 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C.

The 9 species are to be separated based on their differences in volatility, primarily using distillation columns.(benzene,p-xylene, toluene, ethylene, cumene, hydrogen, methane , ethane, propane , propyl) rank the species from most volatile (#1) to least volatile (#9), and what is the physical properties used to make this determination.

Which of the following statements is true?

Fast reactions have small rate constants.

Slow reactions have large rate constants.

A rate equation contains concentration terms for all reactants involved in a one-step mechanism.

A rate equation contains concentration terms for all the reactants involved in a multi-step reaction.

calculate the thermodynamic favorability of aerobic Mn(II) oxidation and aerobic Fe(II) oxidation at pH 2 and 7? Would an organism grow from these processes?

Show all work and don't use previous answers similar to this because they aren't correct. Thanks.

. During the preparation of your dish(chocolate pudding, pasta, bread), the chemical composition of each ingredient plays a role in the texture, aroma and appearance of the final product. Use the table below to describe the chemical composition (molecules, elements, ions, etc.) for the basket ingredients and its corresponding chemical changes and/or physical changes occurring while cooking.  

A)assuming volumes are additive, what volume of water must be added to 28.0 mL of 1.25 M FeCl3 to prepare a 0.650 M FeCl3 solution?
B) what mass of Ca(OH)2 would be required to neutralize 120.0 mL of 0.350 M HClO4? molar mass= Ca(OH)2 74.08; HClO4 100.46
C) what is the minimum volume of 0.08475 M KOH needed to neutralize 10.00 mL of 0.1801 M H2C2O4?
D) a 10.0 L sample of an ideal gas at 25.0°C is heated at constant pressure until the volume has doubled. what is the final temp?

Which Relative Risk (RR) and confidence interval (CI) is most likely to be a causal relationship?

A) RR= 3.0 (95% CI 1.9-7.9)

B) RR= 3.0 (95% CI 0.3-12.2)

C) RR= 1.0 (95% CI 0.3-12.2)

D) RR= 1.0 (95% CI 0.3-4.3)

Part 1: Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 2.80×10-16 at a specific temperature

Part 2; What is the pH of this solution of cobalt(II) hydroxide?

Identify the single most acidic or basic principle species in each of the following solutions. Calculate its molarity or number of moles (your choice). In the case of any species other than H3O+ or OH-, write the net ionic equation for the reaction of that speicies with water. Calculate the pH of each solution.

a) 10.0 mL of 0.30 M HCL

b) 10.0 mL of 0.35 M HF

c) 10.0 mL of 0.25 KOH

d) 15.0 mL of 0.30 M NaOH

e) 15.0 mL of 0.20 M NH3

At 200°C, Kc​ = 1.6*10−10 for: N2​O(g) + NO2(g) ⇌ 3 NO(g). If 350 mL of NO measured at 797 torr and 25.0°C is placed into a 3.00 L container, what will be the molarity of N2​O at equilibrium when the reaction is heated to 200°C? what is the total equilibrium pressure, in units of torr at 200°C?