A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 mL of solution has a pH of 6.02. Calculate the Ka of the acid. __________ x 10^-6
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A solution prepared by dissolving 2.25 g HA (MW = 51.0) and 4.00 g of NaA in 500 mL of solution has a pH of 6.02. Calculate the Ka of the acid. __________ x 10^-6
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- A 25.0 mL sample of 0.250 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) is titrated with 0.250 M NaOH solution. Calculate the pH after the following volumes of base have been added. a. 35.0 mL PLEASE SHOW ALL WORKMaria wants to determine the concentration of Calcium ions in water from their well. She used a 100.0 mL water sample, and its pH was adjusted to 10 and 3 drops of the indicator were added. She used 2.500 mL of 0.09945 M EDTA to reach the endpoint. What is the concentration (mg/L) of calcium ion in the sample? Identify the classification of water given the reference. Reference: 0 to 60 mg/L Ca is classified as soft, 61 to 120 mg/L as moderately hard; 121 to 180 mg/L as hard; and more than 180 mg/L as very hardA 25.0 mL sample of 0.250 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) is titrated with 0.250 M NaOH solution. Calculate the pH after the following volumes of base have been added. a) 0 mL b) 12.5 mL c) 25.0 mL d) 35.0 mL PLEASE SHOW ALL WORK
- find the total hardness for water of lake contains (9.83 x10* ( m) of hco3, (1.25x 10 m) of mg*2,(1.25x10*'m) of ca*2 ,and (0.001 m) co,5. it has a ph value of 105g unknown sodium carbonate titrated with HCl. Two endpoints observed. TITRATION: 20mL of the diluted solution (5g sodium carbonate + 250 water) + 10mL of water were used for the titration (TOTAL VOLUME 30 mL) CO32- + H+ -> HCO3- HCO3- + H+ -> H2O + CO2 First endpoint 45.00mL HCl Second end point 65.00mL HCl FIND: alkalinity of CO32- & HCO3- wt% of CO32- & HCO3- PLEASE SHOW ALL WORKIf a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].
- A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?50.00 mL of 0.1000 M Ti2+ solution is titrated with 0.1000 M Sn4+ solution. Find the concentration of the Ti2+ solution at the equivalence point. K= 4.7x1017 2 Ti2+ + Sn4+ ↔ 2 Ti3+ + Sn2+ A. 8,6 x 10-8 M B. 0,033 M C. 0,0667 M D. 4,3 x10-8 MA 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
- How do you prepare a 1 Liter buffer solution with a pH of 5.0 containing 0.55 M acetic acid and 0.45 M sodium acetate? (Ka: 1.75×10-5)1: An unknown acid (0.596 g) was dissolved in approximately 50 mL of deionized water and titrated with a 0.250 M NaOH solution. When pH vs. Volume of NaOH (mL) added was plotted, the graph below was obtained. The unknown acid is: A) monoprotic B) diprotic C) triprotic 2: What is/are the pKa value(s) for this acid? A) 3.0 and 4.7 B) 4.0 and 7.7 C) 7.7 D) 4.0 E) 4.4 and 11.0 3: The volume of NaOH needed to reach the first equivalence point is: A) 30.0 mL B) 26.0 mL C) 15.0 mL D) 12.5 mL E) 19.5 mL 4: Calculate the number of moles of NaOH used to reach the first equivalence point. A) 0.00750 mol B) 0.00375 mol C) 0.00650 mol D) 0.00313 mol E) 0.00488 mol 5: The molar mass of the acid is: A) 86.9 g/mol B) 104 g/mol C) 66.8 g/mol D) 116 g/mol E) 159 g/molOn titrating 50 ml of 0.01 M KI with 0.01 M AgNO3 . The value of pAg after addition of 30 ml AgNO3 is ...................................................................... ( Ksp= 5.2 xl0 -13 )