A 50.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HBr. What is the most likely pH of the resulting solution after the addition of 60.0 mL of HBr to the NH3? Kp, NH3 = 1.8x10-5

Q: What is the pH of the buffer solution that contains 1.6 g of NH4Cl in 250 mL of 0.060 M NH3? Is the…

A: pH of a basic buffer can be calculated using Henderson-Hasselbach equation: pH=14-(pKb+logB+BOH)

Q: What you expect to observe on mixing 0.1M AgNO3 with 6M NaOH. Will there be a color? Will bubbles…

A: Silver oxide - a displacement reaction occurs, but silver hydroxide isn’t thermodynamically stable…

Q: 21 mL sample of 0.15 M KOH is titrated with 0.125 M HClO4. What is the pH after 23 mL of titrant is…

A: Volume of KOH = 21 mL or 0.021 L  Molarity of KOH = 0.15 M  Volume of HClO4 = 23 mL or 0.023 L…

Q: buffer

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Q: The Kb of ammonia is 1.76x10-5. What is the pH of a buffer which is prepared by combining 50.0mL of…

A: This question can be solved on the basis of the Handerson hasselbach equation which describes the…

Q: Calculate the pH during the titration of 20.0 mL of 0.10 M NaOH (Ka = 1.8 × 10-5) after the addition…

A: NaOH is actually a strong monoacidic base and doesn't need a Ka value.  HCl is also a strong…

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

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Q: 25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have…

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Q: A 1.0-L buffer solution contains 0.300 mol acid, HA, and 0.300 mol base, NaA. The value of K, for…

A: Weak acid and its salt with strong base will make a buffer whose PH can  be calculated with the help…

Q: 4. Calculate the change in pH that results from adding 25 mL of 0.010F HCI to 500ml buffer solution…

A: Given,  [NH3] = 0.25 M  [NH4Cl] = 0.15 M  Volume of the buffer in mL = 500 mL  Volume of HCl added =…

Q: Consider the reaction of a 20.0 mL of 0.220 M C̟H̟NHCI (Ka = 5.9 x 10*) with 12.0 mL of 0.241 M…

A: Given molarity of C5H5NHCl or C5H5NH+ = 0.220 M  Volume of C5H5NHCl solution = 20.0 mL = 0.020 L…

Q: How many grams of sodium hypochlorite, NACIO, need to be added to 227 mL of a 0.185 M solution of…

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Q: A 103.9 mL sample of 0.108 M HCI is mixed with 32.2 mL of 0.088 M NH3. What is the resulting pH?…

A: pH is calculated using formula- pH = -log[H+]

Q: A buffer is prepared from 150 mL 0.185 M NH4Cl (aq) and 200.0 mL 0.105 M NH3. Kb for NH3 is 1.8X…

A: Given: concentration of NH4Cl = 0.185 M concentration of NH3 = 0.105 M Kb for NH3 =  1.8X10-5 Volume…

Q: A 25.0-mL sample of 0.35 M C6H5COOH is titrated with 0.20 M KOH. What is the pH of the solution…

A: The reaction taking place is,

Q: A 98-mL sample of 0.62 M HNO2 (Ka = 4.0 ´ 10–4) is titrated with 0.25 M NaOH. What is the pH of the…

A: Number of mmols = Molarity x volume (mL) Number of mmols of NaOH added = 0.25 x 30 = 7.5 mmol Number…

Q: A 50.0 ml sample of 0.200 M HNO2 (weak acid) is titrated with 0.400 M KOH. Calculate the pH after…

A: Neutralization reaction is a type of chemical reaction that occurs between acid and base resulting…

Q: -1 A 75.0-mL volume of 0.200 mol L NH3 (Kp = 1.8 × 10-3) is titrated with 0.500 mol L HNO3.…

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Q: 10.0 mL of 0.80 M HF is titrated with 0.30 M NaOH. What is the pH of the solution after 10.0 mL of…

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Q: Calculate the pH during the titration of 25.0 mL of 0.100 M NH3 after the addition of 25.0 mL of…

A: NH3 + HClà NH4Cl  PKa = log 5.7 x 10-10 = log 5.7 x 10-10 =9.25 We know on adding NH3 with HCl, NH4+…

Q: A buffer is made using 50.00 mL of 0.7000 M HA (a weak acid, Ka = 1.000 x 10-5) and 50.00 mL of…

A: GIVEN: Initial concentration of HA=0.7000 M  Initial volume of HA =50.00 mL Initial concentration of…

Q: 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: A buffer solution is a mixture of weak acid and its conjugate base or weak base and it's conjugate…

Q: Consider a buffer made by adding 132.8 g of NaC,H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 105)…

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Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCI and 2 drops of…

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Q: What volume of 0.110 M Hydrochloric acid needs to be added to 30 mL of 0.100 M ammonia to make a…

A: We know the Henderson-Hasselback equation is, pH=pKa +salt/acid Given Value;   The concentration of…

Q: A buffered solution containing 0.400 M aniline C6H5NH2 and 0.200 M aniline hydrochloride, C6H5NH3Cl…

A: pH is used to determine the concentration of hydronium ion .

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A: Answer :-               pH = 1.845…

Q: A 100mL sample of 0.20M HF is titrated with 0.10M KOH. What is the pH of the solution after the…

A: HF is a weak monoprotic acid with Ka = 3.5*10-4  KOH is a strong monoacidic base.

Q: You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH;COOH) and 0.30 M sodium…

A: Given: The volume of the buffer solution (V) = 500.0 mL = 0.5 L The concentration of acetic acid…

Q: ) Lead(II) hydroxide, Pb(OH)2 consists of lead(II) ion and hydroxide ion. Given that Kyp value of…

A: Solubility product is an equilibrium constant which is determined by multiplying the concentration…

Q: If 50.00 ml of 1.00M HC,H,O; (K, = 1.8 x 10*) is titrated with 1.00 M NaOH. What is the pH of the…

A: Volume of CH3COOH = 50ml Concentration of CH3COOH = 1M Concentration of NaOH = 1M Ka = 1.8×10-5 We…

Q: Consider a 1.0-L solution that is initially 0.500 M NH3 and 0.570 M NH4CI at 25 °C. What is the pH…

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Q: a. What is the pH of an aqueous solution of 100.0 mL with 1.00 mmol Ca(OH)2 (74.1 mg) dissolved in…

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Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A:

Q: A solution is prepared by combining 20 mL of 0.1M KH2PO4 and 60 mL of 0.1M Na2HPO4 in a 100 mL…

A: pH is used to determine the concentration of hydronium ion.

Q: نقطة واحدة In a titration of a weak acid with a strong base, what is the pH of the solution at the *…

A: Given: Case1: Titration of weak acid and strong base.  Case 2: Some of the titration conditions :…

Q: A student pharmacist prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 mL of 0.12…

A: The working formula is  V1×S1 = V2×S2 V1 = initial volume V2 = final volume S1 = initial…

Q: Determine the resulting pH when 250 mL of 0.35 M HCI is mixed to a 800 mL buffer that has a…

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Q: A titration is performed in which 0.10 M LIOH is added to a 200.0 mL sample of 0.40 M HF. What is…

A: HF is a weak acid it reacts with LiOH which is a strong  base and gives fluoride ion. Now this…

Q: A 40.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HI. What is the most likely pH of the…

A: After addition of 45 ml .1(M) HI to 40 ml .1(M) NH3,the solution does not remain as a buffer…

Q: What is the pH of the buffer solution that contains 1.7 g of NH4Cl in 250 mL of 0.12 M NH3? Is the…

A: The concentration of NH4Cl, [NH4Cl], is calculated as shown below where m is the given mass of…

Q: A buffer is prepared by mixing 204.0 mL of 0.452 M HCl and 0.500 L of 0.400 M sodium acetate…

A: Any particular buffer solution's pH can be derived by Henderson-Hasselbalch expression. Buffer…

Q: 4. A 300 mL buffer is prepared in which [HCO,]= 0.2M and [CO,'] 0.075M a) What is the pH of this…

A: 4. Given that : Volume of buffer = 300 mL [HCO3-] = 0.2 M [CO32-] = 0.075 M

Q: 5.00 mL of 0.100 M ammonia (NH3, K, = 1.8x10 5) is titrated with 0.100 M HNO3. Calculate the pH…

A: Given data: Volume of NH3 = 5 mL Molarity of NH3 = 0.1 M Molarity of HNO3 = 0.1 M Kb of NH3 = 1.8 x…

Q: Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH;CO,K, with 0.207 M HNO3.…

A: Given : Concentration of CH3CH2CO2K = 0.549 M Volume of CH3CH2CO2K solution = 15.75 mL = 0.01575 L…

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 0.240 M pyridine, C,H,N(aq)…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: How many grams of NH4CI would have to be added to 250.0 mL of a 0.420 M NH3 solution to prepare a…

A: The minimum concentration of NH4Cl that must be present in the solution to have a pH of 10 is;…

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.