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- A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)A certain indicator, HA, has a ?a value of 7.9×10^−7. The protonated form of the indicator is yellow and the ionized form is red. What is the p?a of the indicator? p?a= A generic salt, AB2, has a molar mass of 287g/mol and a solubility of 2.80 g/L at 25 °C. AB2(s)↽−−⇀A2+(aq)+2B−(aq) What is the ?sp of this salt at 25 °C? ?sp=A 40.0 mL solution of 0.100 mol/L acetic acid, CH,COOH (K, = 1.8 x 10-5), is titrated with 0.100 mol/L sodium hydroxide at 25 °C. Write the net ionic equation for this titration: %3D NaOH + CH,COOH + CH,COONa + H,0 NaOH + CH,COOH > CH,COONa + H,0 OH- + CH,COOH А. В. C. + CH,COO- + H20 OH-+ CH,COOH → CH;COO + H,0 OH + H* > H20 D. Е. F. OH-+ H* + H,0
- Calculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic sulfuric acid, H2SO4, to a phenolphthalein end-point. Report the answer to a precision of 2 decimal places.A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).21 mL of NaOH is used to reach the endpoint in titrating 0.8001 g KHP (204.22 g/mol). How much of the said NaOH solution will be used in neutralizing 10.00 mL of 0.3245 M H₂SO₄? (Note the stoichiometry of your acid and base) CHOICES: 74.89 mL 37.45 mL 45.00 mL None of these
- A 50 mL portion of an HCL solution requires 29.71 mL of 0.01963 M Ba(OH)2 to reach an endpoint with bromocresol green indicator. Calculate the molarity of the HCl ?Lemon juice contains citric acid which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was neutralized by 15cm^3 of 0.1M sodium hydroxide. a) Calculate; i) concentration of the diluted solution of lemon juice ii) concentration of the original lemon juice. iii) percentage by mass of citric acid in lemon juice.You used 70 mL of deionized water instead of the necessary 50 mL of water to make a KHP solution for standardizing NaOH. What effect would this have on the calculated molarity of the NaOH? A The calculated molarity will be too low. B It is not possible to tell without knowing the volume of NaOH used. C The calculated molarity will be unaffected. D The calculated molarity will be too high.
- 4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.A chemist titrates a 25.0 mL sample of 0.239 M benzoic acid (C6H5COOH) against a 0.100 M solution of NaOH.The overall reaction is shown by the equation below: C6H5COOH(aq)+NaOH(aq)C6H5COONa(aq)+H2O(l) The Ka value for benzoic acid is 6.28 × 10–5. Calculate the pH at the start of the titration, before any NaOH has been added. Give your answer correctly to two places after the decimal.A 0.5027 g of KHP (KC8H5O4; MW = 204.22 g/mol) required 11.90 mL of NaOH titrant to reach the phenolphthalein endpoint. Calculate the standardized concentration of NaOH.