Q 25 mL of a mixture of NaOH and Na 2 CO 3 was titrated with 0.1 HCI using phenolphthalein indicator required 25 mL HCI. The same volume of mixture when titrated with O.1 N HCI using methyl orange indicator required 30 mL of HCI. Calculate the amount of Na 2 CO 3 and NaOH in one .litre of this mixture

Q: What is the pH of a 75.0 ml of a 0.1 M pyridine (C5H5N) solution (Kb= 1.7 x 109) when 100.0 mL of a…

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Q: Classify the given as direct, indirect, or back titration problems. A 50.00-mL sample of a citrus…

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Q: A buffer must be a pH of 10.00 and 750 mL total volume. We have 20 L of 0.20 M NaHCO3 and solid…

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Q: A chemist weighs out 0.338 grams of a unknown diprotic acid into a 122 volumetric flask and makes a…

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Q: Calculate an unknown concentration of a NaOH solution if 0.224 g of oxalic acid, H2C2O4*2H2O,…

A: Molar mass of H2C2O4.2H2O = 126 g/mol Calculation of no. of mol of Oxalic Acid: According to the…

Q: 1.) A 50.0-mL sample of 0.10 M HNO 2 (Ka = 4.0 × 10 −4) is titrated with 0.12 M NaOH. The pH after…

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Q: in an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this…

A: Given that : The mass of Ca = 0.050 g The volume of DI water = 150 mL The molarity of HCl = 0.30 M

Q: A solution containing 2.500 g of a triprotic acid H₂A was titrated with NaOH. It required 45.00 mL…

A: The question is based on the titrations.  We are titrating a weak acid with a strong base. We need…

Q: Grams of diprotic acid Initial buret reading of NaOH(aq) Final buret reading of NaOH(aq) Volume of…

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Q: ralence point. Gi nt (in grams) of t 5738

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Q: A 35.00 mL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1272 M…

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Q: Part A: A 252-mL buffer solution is 0.420 M in ammonia (NH3) and 0.303 M in ammonium chloride…

A: We would use Henderson Hasselbalch equation to calculate  initial pH.  Then , HBr which is a strong…

Q: A 100.0 mL sample of natural water was titrated with NaOH. The titration required 11.43 mL of 0.1539…

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Q: If 15.0 mL of 0.187 M H2SO4 is titrated with 0.132 M NaOH solution, what volume of sodium hydroxide…

A: We can use the molarity equation to calculate the volume of NaOH solution. k x M1V1 = M2V2 Here, M1…

Q: A student performs a titration of 62.0 mL of a phosphoric acid (H₂PO₂) solution of unknown…

A: The question is based on the concept of titration.We are titrating  a weak phosphoric  acid with a…

Q: 2HCl + Ca (OH)2 à CaCl2 + 2H2O Write the balanced net ionic equation

A: The reaction taking place is given as 2 HCl (aq) + Ca(OH)2 (aq) ----------> CaCl2 (aq) + 2 H2O…

Q: a) 50.00 mL of 0.1500 M NaOH is used to titrate 15.25 mL of H3PO4 to the endpoint (neutralization).…

A: The number of moles of a substance is defined as the mass of the substance upon its molar mass. The…

Q: It required 11.96 mL of 0.102 M NaOH to titrate a 0.0927 g sample of an unknown monoprotic acid to…

A: Calculate the moles of NaOH,          (0.102 mol/L) (0.01196 L) = 0.00121992 mol

Q: A 0.500-gram sample of a weak, nonvolatile monoprotic acid, HA, was dissolved in sufficient water to…

A: The molar mass of HA would not be affected by this procedure. Rinsing the buret with distilled water…

Q: In an acid-base titration, how much volume (in mL) of 0.105 M NaOH solution is needed to neutralize…

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Q: 34.19 mL of 0.17 M HNO2 (a weak acid) is titrated with 0.17 M NaOH (a strong base). What volume of…

A: Balanced chemical equation is,HNO2 + NaOH = NaNO2 + H2OAt equivalence point, both reactants…

Q: Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2…

A: From the balanced chemical reaction between HCl and Na2CO3, we can solve these problems. 2HCl +…

Q: In a titration of 36.0 mL of a 0.250 M solution of a triprotic acid H,PO, (phosphoric acid) with…

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Q: Which of the following is the strongest base? The Ka's listed are for the conjugate acid of the base…

A: Since you have asked multiple question as per our company guidelines we are supposed to answer the…

Q: A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is…

A: A solution which is a mixture of weak acid and its conjugate base is known as buffer. For…

Q: A student completes a titration of an unknown diprotic acid. In this experiment, 0.79 g of the acid…

A: Step 1: Step 2: Step 3: Step 4:

Q: 10.00mL of 0.10M HCI were collected in an Erlenmeyer flask, and then diluted to 100mL with distilled…

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Q: 4. Calculate the pOH when 35.0 ml of 0.650 M HF is mixed with 15.0 ml of 0.125 M KOH. K, = 7.1 x 10*…

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Q: 15.84 mL of 0.250 mol/L phosphoric acid was titrated into 10.00 mL of magnesium hydroxide.…

A: Phosphoric acid is a polybasic acid.   The reaction will be:-  2H3PO4+3Mg(OH)2→Mg3(PO4)2+6H2O

Q: 10. mL of 0.25 M Ca(OH)2 solution is titrated with 0.50 M HNO3 solution, calculate pH of the…

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Q: An analytical chemist weighs out  0.019g  of an unknown monoprotic acid into a  250mL  volumetric…

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Q: A student performs a titration of 31.0 mL of a phosphoric acid (H3PO4) solution of unknown…

A: Given,

Q: A 100.0 mL sample of natural water was titrated with NaOH. The titration required 13.25 mL of 0.1589…

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Q: 25.0-mL sample of 0.100M Ba(OH) 2 is titrated with 0.125M HCl. How many milliliters of HCl will be…

A: Interpretation: A 25.0 mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. The volume of HCl…

Q: How many liters of pure water will be required to disslove 0.885g of solid lead iodate, if the water…

A: First the moles of Pb(IO3)2 present in given grams is calculated as below,Water already contains…

Q: An analytical chemist weighs out 0.118 g of an unknown triprotic acid into a 250 mL volumetric flask…

A: Mass of the triprotic acid = 0.118 g Volume = 250 mL Molarity of NaOH = 0.1100 M Volume of NaOH…

Q: Given the following data, calculate the grams of HCl neutralized in the titration using 0.250 M…

A: Ans is 0.1449g

Q: When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the…

A: ANsweR: We’ll answer the first question since the exact one wasn’t specified. Please submit a new…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.