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Q: calculate the milltifres of 0-250M Naz PO that win reget with 30.0mL of O•250 M MIC12 •
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- A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/molPhenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
- A 3.00 mL aliquot of 0.001 M NaSCN is diluted to 25.0 mL with 0.1 M HNO3. How many moles of SCN- are present?Q1) A sada- Lime Sample is 90% NaoH and 10% CaO• If 3gm is dissolved in 250 ml, what is the tutal normadity of the Selution as abase ? How many milliliters of O.57N H2 S@4 would be requiredd to titrate i00 me of the Solution ? Ans.s ( 0.309 N, 60.59 ml) Q12) How much water that required add to 200 ml HNO, ( densly = 1.285 gm/ml) Contains 46 wt% acid to Convert lo wt% acid solution? Ars. : 919.6 mlThe pH of a Buffer containing 1.OM CH3COOH and 0.1M CH3COONA (pka of * :CH3COOH =4.74) is 3.0 4.74 3.74 5.74
- 3. Cal culate Nattz POy:(Ka, kaz and tas of HsPO4 6.32x10-8 and 4.5x10-13 he ott of a o.0400M Shutin of ane 7.11 メL65 respectively). 4. Con Sider the titration of 1w.00ml of a 0.200M Solution of he hypothetical acid tzA uith o.loc Soclium hydroxide. Enourhg hat Kay = (. 00 k1o-8, and kag = 1.00 xLo 12 Calculate ka after he addition of a) 1o. oml Na OH =l:00x16", E1:00x104 9 20.oml Na OH ) 30. omL Na ott d) 40.0ml Na OHI1.6. A lo0mL solntion g 0.050MM tuffered to pHq.00 was titrates rith n+ 0. OSD OMEDTA. ca) Hhat is the egniralene volume, Ve in milliliters? (b) Caleulate Hhe concenpration f m" at ntA 0.5000 g sample contains NaHCO₃, Na₂CO₃ ,and NaOH, either alone or in permissiblecombination. Titration of a 50.0-mL portion toa phenolphthalein end point requires 25.1 mLof 0.100 M HCl. A second 50.0-mL aliquotrequires 50.2 mL of the HCl when titrated to abromocresol green end point. Deduce thecomposition, and calculate the percentcomposition of the substances. Find the mmol of Na2CO3, g of Na2CO3, and concentration of Na2CO3.
- 3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124Titration purity NxVx mEq weight weight of sample (g) x 100 Volume (Weight of sample (g) Nx mEw Weight V = 100 Normality Weight of sample (g) Vx mEw Weight N = 100 mEq Weight mEq Weight % x Weight of sample (g) V xN /100 Weight of sample Nx Vx mEq weight (9)= x 100 %3D % Purity Volume 2 Normality 1 Normality 2 Volume 1The Merck Index indicates that 10 mg of guanidine,CH5N3, may be administered for each kilogram of bodymass in the treatment of myasthenia gravis. The nitrogenin a 4-tablet sample that had a total mass of 7.50 g wasconverted to ammonia by a Kjeldahl digestion, followedby distillation into 100.0 mL of 0.1750 M HCl. Theanalysis was completed by titrating the excess acid with11.37 mL of 0.1080 M NaOH. How many of thesetablets represent a proper dose for a patient who weighs(a) 100 lb, (b) 150 lb, and (c) 275 lb?