The pH after adding 23.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is   0.080   1.1   1.4   0.042

Q: A scientist dilutes 50.0 mL of a pH 5.85 solution of HCl to 1.00 L. What is the pH of the diluted…

A: Given data,pH=5.85Volume of HCl=50mL=0.050LDilution=1.0LKw=1.0×10-14

Q: If we have a solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs to be…

A: Hey, as the volume of weak acid is not given in the question, I consider it as 25 mL in order to…

Q: 8. What is the PH of a solution with [H*]=1 x 10-³M ]3 2HCNO ]-3HF |-2 ]None of the others 9. What…

A: Hello. Since more than one question has been asked, the first question shall only be answered in…

Q: Which of the following solutions will have the lowest pH value? Group of answer choices 0.10 M HNO3…

A:

Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: Given the Kb of C6H5NH3+ is 3.98x10-10 : 1.) What is the [H3O+] concentration in a solution that is…

A: Given,  Given the Kb of C6H5NH2  is 3.98x10-10 : The [H3O+] concentration in a solution that is…

Q: How many gram of ammonia should be added to 500mL of 1M ammonium chloride to give a pH 9? Ka…

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Q: aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10–14) 0.020 M HNO3

A: As we know,  Acidic solution has pH less than 7. Basic solution has pH greater than 7 . pH =…

Q: What is the pH of a solution that is 0.12 M in HOCl and 0.20 M in NaOCl?  Ka of HOCl is 3.5 x 10-8…

A: Given, 0.12 M in HOCl and 0.20 M in NaOCl

Q: What is the pH of 10.0 mL of 0.0020 M HCl?     3.70     10.0     5.70     2.70     0.70

A: Given the on concentration of HCl solution =  0.0020 M The pH of 10.0 mL of 0.0020 M HCl =

Q: 1. write the dissociation equations for each substance and calculate the pH. a) 0.0035 M HClO4 b)…

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

Q: Penicillin (MW = 356) is an antibiotic often used to treat bacterial infections. Its acid ionization…

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Q: Determine the pH of 80 mL of a 0.30 M solution of acetic acid when 0, 40 mL, 80 mL and 100 mL  of…

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Q: A titration of 0.100 M NaOH is titrated into 25.0ml of a 0.100 M HCHO2 solution (Ka = 1.80 x 10 4).…

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Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

A:

Q: A solution is prepared by dissolving  1.600 g  of sodium acetate (CH3COONa) into  100.00 mL  of a…

A: • pH of weak acid can be calculate by      the help of Hendenson - Hasselbalch equation:-pH=pka +…

Q: What is the pH of a 0.15 M HOCl solution (Ka = 3.0 x 10-8)

A: HOCl is weak acid hence it dissociated less in solution

Q: What is the pH of 0.1000 M Na₂HPO4? (K₁2=6.2x10-8, K3=4.8x10-13) What is the pH of 0.1000 M Na3PO4?…

A: The solutions considered are 0.1000 M Na2HPO4 and 0.1000 M Na3PO4. The question requires to…

Q: What will be the pH of 0.025 M NaOH solution in H2O at 60 °C? (KW60°C = 1.0 x 10-11) A. 1.6 B. 9.4…

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Q: Complete the following statements about the below solutions at 25 °C? 1. The pOH of 9.95 x 105 M KOH…

A: at 25°C ;  pH + pOH = 14.0  pOH = -log[OH-]

Q: 19.00 mL of 0.100 M sodium hydroxide is added to 39.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Since sodium hydroxide is a strong base.  hence it will react with the acetic acid as  NaOH +…

Q: for hypochlorous acid, HClO, is 3.0×10-8. Calculate the pH after 40.0 mL of 0.100 M NaOH have been…

A: Ka(HClO) = 3.0 × 10^-8 Volume of NaOH = 40.0 ml Molarity of NaOH = 0.100 M Volume of HClO = 40.0ml…

Q: Find the pH of the following acidic solutions: A 0.001 M solution of HCl (hydrochloric acid). 3…

A: 'As you have posted multipart question, we will solve first three. If you want any specific part to…

Q: The pH of a 0.25 M aqueous solution of HF at 25°C is 2.03. What is the value of Ka for HF?     3.7…

A: pH gives the information about the acidity or alkalinity of a solution. pH is determined from the…

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: What is the pH of a 0.25 M F- solution (Kb = 1.4 x

A: Given,   Concentration of Base = 0.25 M Kb = 1.4 ×10-11 pKB = -Log(Kb)   = -log(1.4×10-11) = 10.85

Q: What is the concentration of hydrogen ion in a solution with a pH of 5?     1×1051×105 M 1 times 10…

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Q: For each of the following cases, decide whether the PH is less than 7, equal to 7, or greater than…

A: Moles = Concentration X volume of solution in L

Q: What is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? The Ka of propionic…

A: Sodium propionate is a salt of weak acid and strong base. Given, Ka of propionic acid = 1.3x10-5…

Q: A 1.0 × 10 -2  M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of? 12.30     12.00     2.0 ×…

A: Answer:- This question is answered by using the simp[le concept of calculation of pH of the solution…

Q: Arrange the following solution from lowest pH to highest pH: 0.75 M CH3COOH (K, = 1.8 x 10-5) 0.01 M…

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Q: Which of the following has the lowest pH?   3.9x10-3 M HPO42- (Ka3=4.2x10-13)   0.00010 M H3BO3…

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Q: Acetic acid is a weak acid with Ka = 1.8 x 10 -5 and ionizes into HC2H3O2 -------H + + C2H3O2 - What…

A: pH is negative logarithm of hydrogen ions

Q: Calculate the pH of a solution when 32.0 mL of 0.200 M formic acid (HCOOH, Ka = 1.77 x 10-4) is…

A:

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…

A: Given data,Molarity of NH3=0.15MVolume of NH3=50mL=0.050LMolarity of HCl=0.20 MVolume of…

Q: After dissolving 0.35 g of magnesium hydroxide in 135 mL of water, how many mL of a 1 L hydrochloric…

A: M= n / V(in L)   where   n = moles of solute (Mg(OH)2) = mass / molar mass = 0.35 g / 58 g/mol   =…

Q: Arrange the following solution from lowest pH to highest pH: a) 0.20 M CH₃COOH (Ka = 1.8 x 10⁻⁵),…

A: (a) First of all First of all the ICE table has to be drawn for the dissociation of acid as:…

Q: Consider the following data on some weak acids and weak bases HNO2 Ka 4.5x10^-4 HCH3CO2 Ka…

A: Larger the value of Ka, more acidic is the compound and lower is it’s pH (pH< 7). Since Ka of…

Q: When 25.0 mL of 0.200 M hydroiodic acid and 25.0 mL of 0.200 M ammonia are combined, the pH of the…

A:

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

A: The strength of an acid depends on the extent of its dissociation in water. Strong acids dissociate…

Q: Find the pH of a 0.4M aqueous hydrocyanic acid solution. For HCN, Ka=4.9 x 10^-10     4.85…

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Q: Ka for a 0.100 M methanoic acid solution whose pH is 2.37 is   4.2x10-3   8.7x10-3   1.8x10-4…

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Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10^-4. What is the pH to 2 decimal places when 13.75…

A: Given : Ka=7.2×10-4 Volume of KOH=13.75 ml Molarity of KOH=1.074 M Volume of HF=27.5 ml…

Q: Calculate the pH of a 0.20 M C2H5NH2 solution. Kb=5.6x10-4

A: C2H5NH2 is a weak base. pH of this solution  = 12.04

Q: In the laboratory, a general chemistry student measured the pH of a 0.429 M aqueous solution of…

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Q: What is the pH of a solution made by adding 0.65 mol of acetic acid (H3CO2H) and 0.30 mol of sodium…

A: Given : solution with weak acid i.e acetic acid moles = 0.65 mol And conjugate base salt of weak…

Q: What was the original concentration (M) of an aqueous acetic acid (CH3COOH) solution whose pH is…

A:

Q: What is the pH of a solution prepared by dissolving 8.13 grams of NaCN (49.01 g/mol) in 1.4 L of…

A: Given,  The pH of a solution prepared by dissolving 8.13 grams of NaCN (49.01 g/mol) in 1.4 L of…

Q: Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M NaCN with (a) 4.20 mL of 0.438 M…

A: You have posted 2 different  questions simultaneously, so I have to solve the first one that is 5…

Q: Trimethylamine, (CH3)3N, is a gas with a fishy, ammonia–like odor. An aqueous solution that is 0.29…

A: The ionisation reaction of (CH3)3N is  (CH3)3N (aq) + H2O (l)  ------> (CH3)3NH+ (aq) + OH-

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.