A 1.4350-gram of KHP (actual formula = KHC8H4O4; molar mass = 204.22 g/mol) was dissolved in 50.00 mL of deionized water. The resulting solution was titrated with NaOH solution of unknown concentration. If 32.85 mL of the NaOH solution was required to reach the equivalent point, what was the molar concentration of the NaOH solution? The acid-base reaction is as follows:                 KHC8H4O4(aq)  +  NaOH(aq)  -->   NaKC8H4O4(aq)  +  H2O(l)          (A) 0.1405 M           (B) 0.2139 M           (C) 0.08481 M           (D) 7.0267 x 10–3 M

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

A chemistry student weighs out 0.0827 g of phosphoric acid (H,PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0600M NaOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL FEB 19 ... MacBook Air DII 80 888 F10 F7 FB F9 F4 F3 %23 %24

If 40.0 g of C₂H₅OH (MM = 46.07 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of C₂H₅OH in the resulting solution?

A student is given 0.716 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.430 M NaOH. The equivalence point is reached when 37.0 mL are added. Answer the following questions to determine the identity of the unknown acid. -How many moles of NaOH are consumed? Moles of NaOH = ____ mol -How many moles of H+ acid are available to react if the acid is H2C2O4? 0.0403 mol NaOH Moles of H+ from H2C2O4 = ___ mol -How many moles of H+ are available to react if the acid is H3C6H5O7? 0.0403 mol NaOH 0.0573 mol H+ from H2C2O4 Moles of H+ from H3C6H5O7 =  ___ mol

A 5.00-mL sample of vinegar was pipetted into a flask, two drops of phenolphthalein indicator were added, and the acid was titrated with 45.62 mL of 0.1008 M NaOH. If the density of the pipetted acetic acid solution was 1.004 g/mL, what was the percentage of acetic acid in the sample? MW HOAc =60.1 g/mol

25.0 mL Ca(OH)2 solution was titrated with 3.58 mL HCl. The average concentration of HCl is 0.1927 M. What is the concentration of Ca(OH)2?

A chemistry student weighs out 0.106 g of ascorbic acid (H,C,H,O), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NAOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL 19 MacBook Air DII 888 F6 F7 F8 F4 F5 F3 &

A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask.  After the addition of methyl orange, a titration with 0.0045 M HCl was performed.  The endpoint was reached after 8.72 mL of the acid was added.   What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction?  What is the molar concentration of hydroxide in the saturated solution?  What is the molar concentration of Magnesium ion in solution?

2. To standardize a solution of NaOH, a student measured 0.326 g of potassium hydrogen phthalate (KHC8H404 or KHP) and dissolved it in 50.0 mL of water. To the solution, two drops of phenolphthalein indicator was added. To reach the equivalence point as indicated by endpoint of the titration where the solution retained a pale pink color, a volume of 15.3 mL was required. What is the molarity of the NaH solution? (KHP is a monoprotic acid that furnishes one H* ion; at the equivalence point, mols OH (base) = mols H* (acid))