1.) Commercial contcentrated aqueous ammonia (NH 3 ) is 28.0% ammonia by mass & has a density of 0.9000 g/ml What is the molanty of this solution? What is the moality?
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- A stock solution has a concentration of 3.04 NE tf 29.4 mt. of the stack solution is cliluted to a total volume of 180 ml, what is the final concentration (in MP50X TBE is 87 mM Tris-borate and 4 mM EDTA at pH 8.3. What is the molarity of each of the chemicals in 1X TBE buffer?fill in the volumes required to make the various dilutions of Coomassie Blue and their respective concentrations. show sample calculations.
- In order to make a solution of the concentration 0.364 M, what mass of NaCl should bedissolved in 152 mL of water?Calculate pH of buffer prepared by mixing; 10ml of 0.10M of CH3COOH and 20ml of 0.10M of CH3COONa.2) Calculate the pH during the titration of 20.00 mL of 0.1000 M butanoic acid (K,-1.54x10%) with 0.1000 M NaOH solution after the following additions .0 mL .10.00 mL 15.00 mL 19.00 mL .19.95 mL . • 20.00 mL • 20.05 mL . 25.00 mL
- A buffer solution contains an equal concentration of weak acid HX and its conjugate base ion X™. The ionization constant Ka of HX is 2.2 x 10-8. What is the pH of the buffer?A 35 mL of solution of hydrochloric acid is neutralized by 15 mL of 0.5 M potassium hydroxide. What is the concentration of hydrochloric acid? The balanced equation is HCI + KOH - H,O + KCI O 0.75 M O 0.25 M O 0.214 M O 0.786 MDraw titration curve for compound X when NaOH equivalence(s) is/are added. Indicate the buffering region(s) with a box.
- An aqueous solution contains 0.34 M potassium cyanide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.34 mol HCI04 0.16 mol NaOH 0.33 mol KCIO4 0.16 mol HCIO4 0.33 mol HCNWhat is the pH of a buffer that contains 0.9 M ammonia and 0.3 M ammonium ion? (Ka for ammonium ion = 5.8 x 10-10How much water must be added to 300 mL of an aqueous solution of 0.2 M acetic acid in order to double the degree of ionization? Take the acid ionization constant of acetic acid to be 1.8 x 10-5.