AMT (ammonium meta tungstate) has a MW of 2956.2 g/mol. Calculate the amount of AMT (in grams) needed to be dissolved in water that would give a 0.2 M AMT aqueous solution. Also on an unrelated problem, how would you dilute (with water) 12.1 Normality HCl and 14.8 Normality NH4H2O to give 1M HCL and 1M NH4H20 respectively?
Solution X in water has [H+] = 1.0x10-2M Solution Y in water has [H+] = 1.0x10-5M A. Which solution is more acidic ? B. What is the pH of solution X ? C. What is the pH of solution Y ? D. What is the [OH-] of solution X ?
Hello, I need help figuring these problems out! Thanks :-) 1. Balance the following equations: a. P4(s) + 02(g) --> P4O10(s) b. Fe2O3(s) + C(s) ----> Fe(s) + CO(g) c. C4H10(l) + 02(g) --> CO2(g) + H2O(g) + energy 2. Aluminum metal reacts with bromine gas to produce aluminum bromide. a. Write a balanced equation, incl
What is the ph of a 50mM TRIS solution prepared from TRIS acid (157 MW, pKa = 8.3 at 20 degrees C? Do I use the H-H equation. I was confused on this b/c it does not state how much of the acid or base?
Calculate the pH at the equivalence point for the titration of 1.0 M ethylamine, C2H5NH2, by 1.0 M perchloric acid, HCIO4, (pKb for C2H5NH2 = 3.25)
1. Analyze and explain the buffer system in buffered aspirin (carboxylic acid). 2. State three examples each of acids, bases, and salts commonly used in therapeutic processes. From the examples you state, select one acid, one base, and one salt and describe how and where they are used in therapeutic processes. Please
Discuss in detail the healthcare applications of chemical reactions. Which chemical reactions would you consider to be of importance to healthcare professionals? Why? In which situations are these chemical reactions useful to healthcare professionals? Please include references if need be. Thanks
Even through the para position is on carbon father from the carboxy group than the meta position, p-cyanobenzoic acid is more acidic than m-cyanobenzoic acid. Explain the differences in acidity between p-cyanobenzoic acid and m-cyanobenzoic acid.
Oximes are usually crystalline materials and have been prepared as a means of identifying liquid ketones or aldehydes. It has been found in the preparation of these derivatives that if the concentration is too high (low pH), that the oxime does not form. Explain.
Calculate the pH of CO2-saturated water at 25 degrees C, given that the CO2 concentration in air is 343 and that for carbon dioxide the Henry's Law constant KH=3.4E-2 mol L-1 atm-1 at 25 degrees C. Furthermore, the ionization constant, Ka, for H2CO3 has a value of 4.5E-7 mol L-1 at this temperature.
For a molecule of fluorous acid, the atoms are arranged as HOFO. What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. Two possible electron-dot structures are shown for the cyanate ion,NCO- . What can you conclude about how favorable the structures are? a) Str
I need help preparing an IV solution. I have all the ingredients below in solid form, and plenty of sterile distilled water. I need to prepare a solution so that each liter contains the following ingredients at the following concentrations. 0.03 M Galactose 40 millimoles Fructose 50 milliev. lactose 0.008 M Magnesium Phosp
1. Draw all relevant resonance structures for the conjugate base or base. 2. Predict where the 3 compounds would be relative to this order. 3. Explain your reasoning for your predictions. I have attache the structures and the questions. Thanks
Solid magnesium carbonate reacts with an aqueous solution of perchloric acid what is the net ionic equation for the below balanced equation? MgCO3(s)+2HClO4(aq)>>Mg(ClO4)2(aq)+H2O(l)+CO2(g)
1. Provide two examples each of an acidic oxide and a basic oxide. For each example (four in all) write a balanced reaction equation with water to support your claim. a. Acidic oxide 1 Reaction with water b. Acidic oxide 2 Reaction with water c. Basic oxide 1 Reaction with water d. Basic oxide 2 Reaction with wate
Calculate the pH of the 0.32 M NH3/0.35 M NH4Cl buffer system. I think i was near the right anwser with 4.71 but this was wrong. Should i assume that the buffer system is in equlibrium at 80 mL? What is the pH after the addition of 20.0 mL of 0.050 M NaOH to 80.0 mL of the buffer solution?
Calculate the pH at the equivalence point in the titration of 66 mL of 0.10 M methylamine with a 0.20 M HCl solution. i found the kb of Methylamine to be 4.4 X 10^-4. but you use the ka of CH3NH3+ which is 2.3 X 10^-11. I thought it should be 10.94 but its incorrect.
Exactly 100 mL of 0.20 M nitrous acid (HNO2) are titrated with a 0.20 M NaOH solution. Calculate the pH for the following. (a) the initial solution 2.02 is correct (b) the point at which 80 mL of the base has been added 2.44 is incorrect and differs from the correct answer by 10% to 100%. (c) the equivalence point
HNO3 versus CH3NH2. I thought it should be bromophenol blue and methyl orange but this is wrong... what am i doing wrong? i also thought it might be chlorophenol blue but this is incorrect aswell.
(a) Calculate the pH of the 0.20 M NH3/0.18 M NH4Cl buffer. for this part i got the wrong anwser of 9.21 so im not sure how to even begin part b (b) What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 70.0 mL of the buffer?
Lab: Standardization of NaOH Solution Procedure !: 1. Prepare the NaOH solution by dissolving approximately 4g of solid NaOH in 200mL of water in a 250mL beaker. Calculate the approximate NaOH concentration: a. Convert grams of NaOH to moles of NaOH (MW = 40.00, moles = g/MW) b
What is the pH of 380.0 mL of an aqueous solution containing 0.523 g of the strong acid trifluoromethane sulfonic acid (CF3SO3H)? I dont know how to find the Ka of sulfonic acid or do I even need it to solve for the pH?
What are the concentrations of HSO4-, SO42-, and H+ in a 0.35 M KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4- = 1.3 10-2.) I've tried .085 for HSO4- and .054 for H+.... what am i doing wrong? Im getting confused because the tables in my chem book dont have a Ka value for KHSO4
Hydrofluoric acid,HF (aq) , cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF (aq) . Sodium silicate (Na2SiO3), for example, reacts as follows: Na2SiO3(s)+8HF(aq)>>H2SiF6(aq)+2NaF(aq) - How many moles of HF are needed to react with 0.330 mol of Na2SiO3? - How many
A 0.040 M solution of a monoprotic acid is 14 percent ionized. Calculate the ionization constant of the acid. How do I integrate these two equations to solve this problem? percent ionizations = ionized acid concentration @ equilibrium/initial concentration of acid & Ka= ([H3O+][A-])/[HA]
The empirical formula is CH2O the compound is 40% C, 6.70%H and 53.3% O and assume we have a 100g sample of it. question: the molecular formula mass of this compound is 90.0 amu. What are the subscripts in the actual molecular formula?
Chemistry Lab Procedure: 1. Take a burette from the glassware shelf and place it on the workbench. 2. Fill the burette with 50mL of 0.2M potassium permanganate solution. Record concentration. 3. Take flask and add 10mL of New hydrogen peroxide (New H2O2). 4
[about 100 words] Explain in molecular terms the difference between a strong acid and a weak acid, and between a strong base and a weak base. [about 100 words] Explain the physical properties of a strong acid and a weak acid.
In order to do the following problem, do I subtract the Kc from each other? The following equilibrium constants have been determined for hydrosulfuric acid at 25°C. H2S(aq) = H+(aq) + HS -(aq) K'c = 9.5 10-8 HS -(aq) = H+(aq) + S2-(aq) K"c = 1.0 10-19 Calculate the equilibrium constant for the following react
How do I complete this table? Sodium hydroxide H = 4.2 x 10^-10 OH = _______ pH = _______ pOH= ________ Hydrocloric Acid H = _________ OH = _______ pH = _______ pOH= 11.5 Potassium Hydroxide H = _________ OH = _______ pH = _______ pOH= 2.5 Acetic Acid ka=1.8 x 10^-5 H = _________ OH = 6.3 x 10^