2 The artificial sweetener Saccharin (shown below) is a weak acid (pk.-2.32 at 25°C), It is...
2. Saccharin is a common artificial sweetener without calories. When 3.00 g of the sodium salt of saccharin (the anion of saccharin with a Na cation) is dissolved in 50.0 mL of water, it takes 14.6 mL of 1.00 M HCl to reach the equivalence point. Using the data provided, calculate the molecular weight of sodium saccharin?
1. Saccharin is an artificial sweetener that was discovered in 1879 when a chemist spilled some of his product on his sandwich, and when he ate his sandwich discovered it was particularly sweet. It is synthesized according to the following reaction and the product is isolated after addition of HCI. -NH₂ + NaOH + KMnO4 NH OS=0 a) What safety rule did our chemist violate when discovering saccharin? (1 pt) b) Redraw the structure of the carbon-containing starting material, explicitly...
ADDS AND BASS Calculating the pH of a salt solution Calculate the pH at 25°C of a 0.30 M solution of sodium hypochlorite (Nacio). Note that hypochlorous acid (HCIO) is a weak acid with a pk of 7.50. Round your answer to I decimal place. | pH=0
3. Consider the following weak acids and their K, values, calculate the pK, for each acid. HC,H,O, - Acetic acid K. = 1.8 x 105 PK,= H,PO, - Phosphoric acid K = 7.1 x 10 PK, HCIO - Hypochlorous acid K = 3.5 x 10 pk = You want to prepare buffers at pH 2.8, 4.5 and 7.5. Which weak acid-conjugate base buffer system is the best choice for each pH from the acids listed? Write the reaction and indicate...
In a titration, 25 mL of 0.10 M weak diprotic acid solution was titrated by 0.10 M sodium hydroxide, NaOH, and produced a titration curve listed below. (20 points total) 14,0 3. 12.0 10.0 8.0 pH 6.0 4.0 2.0 10.0 5.0 20.0 30.0 15.0 25.0 Volume of 0.100 M NaOH, mL The acid used in above titration is a weak diprotic acid. Briefly explain how you know it's diprotic from looking at the titration curve and how you know a...
2) Draw the 2 reactions of the weak acid, Carbonic Acid (H2CO3) with water. Which form of carbonic acid predominates at physiological pH? The two pKas of carbonic acid are the following: pK,1 = 6.4 pK,2 = 10.3. (3 points) 3) You have a 0.1 M solution of HCl in water. HCl is a strong acid. What is the pH of this solution? (Show your work or will not receive credit.) (2 pts.) 4) Calculate the pOH of a solution...
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M 25 mL of the week acid into 100 mL beaker titrated this solution of 0.21 M NaOH moles of weak acid = 3.75*10^-3 moles of NaOH = moles of week acid c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
please answer number 5 and 6 5. The buffer range for a given weak acid/conjugate base pair is pK, 11. Explain why. 6. A weak triprotic acid, HZZ has the following K, values: Ki = 1.4 x 104 K = 9.7 x 10-7 K 5.3 x 109 a. Write the NIE associated with each Ka value. b. Of the four weak acid species: H.Z, H,Z, HZz"; which two could be used to prepare a buffer of pH = 3.55? Explain....
Titration curve for a weak acid l pH-pK, + log(İHAİ IA I 3. After class practice: calculate the pH of 25.0 mL of 0.100 M formic acid solution (HCOOH: pK 3.74) after you add: iet Show calcuktions A. 10.0 mL NaOH added B. 12.5 mL NaOH added C. 15.0 mL NaOH added D. 20.0 mL NaOH added Half-equivalence point (pH pKa) 14 12 10- mol CHO2 0.00100 Volume (mL) 10.0 12.5 15.0 20.0 mol HCHO2 0.00150 0.00125 0.00100 0.00050 pH...
in (acetylsalicyclic acid HCH,04) is a weak acid. It ionizes in water according to the following equation HC,H,O4(aq) + H2O + H20aq) + CH-07 (aq) 0.10 M aqueous solution of aspirin has a pH of 2.27 at 25°C. Calculate K, for the aspirin (Hint: Use ICE chart). (5) I 0.1 OM с - х E 0.10 - X 8. A certain acid was found to have a pk,=4.88. What is the K, for this acid? Is it stronger or weaker...