Question 7.Calculate the expected pH of the DI H2O + 1.0 mL of 1M NaOH *(The final volume after the addition of NaOH is 51 mL)*

Q: Show that adding 1.0 mL of 0.10 M HCl changes the pH of 100 mL of a 1.8 × 10−5 M HCl solution from…

A: In the above problem , we need to find the pH of 100 mL of a 1.8 × 10−5 M HCl solution, and then the…

Q: How many grams of NaIO (Kb (IO-)=5x10-4 ; MW=213.9 g/mole) must be added to 40.0 ml of 0.1 M HCl to…

A: pOH = pKb + log [NaIO]/[HOI] pH = 14 - pOH

Q: Find the pH of a solution made by mixing 14.0 mL of 0.15M HNO2 and 18.2mL of 0.12M NaNO2

A: HNO2 is weak acid and its conjugate base is NaNO2. So, HNO2 and NaNO2 form a buffer solution.  using…

Q: You are given an HI solution at pH 1.3. How much water do you need to add 0.050 L of this solution…

A: ⊙we know,   PH=-log[H+]⇒[H+]=10-PH⊙concentration=no.of molesvolume⊙No. of moles= concentartion *…

Q: Calculate 3OH-4 and pH for 1.00 mL of 0.175 M NaOH diluted to 2.00 L

A: The formula used to calculate pH: pH=-log(H+). Given data: Concentration of NaOH is 0.175M. Volume…

Q: 4. Calculate the pH of a 0.47 M solution of HOI. (Ka= 2.3 x 10-11). Use 2 decimal places in your…

A: 4. For weak acid, pH = 1/2 pKa- 1/2 Log C

Q: 4. At 40.°C the value of Kw is 2.92 x 10-14. a. Calculate the [H*] and [OH] in pure water at 40.°C.…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: Would you need NaOH or HCl to bring the pH of 0.050 0 M HEPES to 7.45?

A: HEPES is (4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid). It is a zwitter ion buffering agent.…

Q: hich of the following statements are TRUE? Multiple answers:Multiple answers are accepted for this…

A:

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.186? 6.52 -…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What volume of water must be added to 40.0 mL of NaOH solution having pH 13.00 in order to produce a…

A:

Q: What is the pH if I mix 20.0 mL of 0.100 M HAc, 30.00 of .100 M NaOH, and 20.0 mL of distilled H2O?

A: pH is the measure of acidity or basicity of a solution.  Mathematically, it is the negative…

Q: What is the mass of NaOH that would have to be added to 500 mL of a solution of 0.20 M acetic acid…

A: We have : Volume of solution= 500 ml Molarity of acetic acid= 0.200 M ph of the solution = 5.0   Let…

Q: Calculate the volume of NaOH 0.50M needed to obtain a 1:1 acid:acetate ratio from 50mL of acetic…

A: Given,  The volume of 0.50 M NaOH needed to obtain 1:1 acid:acetate ratio from 50mL of 0.20 M acetic…

Q: Using Henderson-Hasselbalch equation, calculate how much volume of 1M HCL is needed to bring down…

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Q: 1. Complete the reaction Mg(OH)2 Mg+2 +2 ionization 2. What is the pH of a 0.001000 M Mg(OH)2…

A: The reaction given is, =>

Q: Calculate the hydronium and hydroxide ion concentration at 25°C in a. 0.15 M H2SO4 b. 8.4 × 10−3 M…

A: For aqueous solution, the product of the concentration of hydronium and hydroxide ions is given by:

Q: 1. The Ka of boric acid, H3B03, is 5.8 x 10-10. Calculate the [H*], [OH¯], pH, pOH, Kb and percent…

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Q: Questions 30 and 31 both involve a 0.22 M solution of acetic acid (CH3COOH). Tme Ka of CH3COOH is…

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Q: Calculate the pH after 0.047 mole of NaOH is added to 1.00 L of each of the following solutions.

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Q: What is the calculated pH of the initial 0.100M Acetic Acid solution?  Ka = 1.8 x 10-5 .  Give your…

A: The dissociation reaction of acetic acid is given below: CH3COOH(aq) + H2O(aq) ⇌ CH3COO-(aq) +…

Q: 2,What is the pH of the solution with  hydronium ion concentration of 6.3 x 10-12 M? Group of…

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

Q: True or False. Write TRUE if the statement is correct and FALSE if it is incorrect. ___________1.…

A: 1. False,  higher the pH, lower is the acidity  2. True 3. True

Q: Find the ph and the percent hydrolysis of a 0.0335 M solution of pyridine hydrochloride (the salt of…

A: Given : Concentration = 0.0335M

Q: acid base K K₂b name formula name formula 10 nitrous acid HNO₂ 4.5 x 10 aniline |C HạNH, | 4.3 × 10…

A: Ka value of acetic acid = 1.8×10-5 Ka value of HNO2 = 4.5×10-4 Kb value of aniline = 4.3×10-10…

Q: 45 Calculate [OH] and pH for (a) 1.5 × 10³M Sr(OH)2, (b) 2.250 g of LIOH in 250.0 mL of solution,…

A: pH of the solution depends on concentration of H+ ion and pOH of solution depends on concentration…

Q: What is the pH of a solution that is 0.26 M CH3NH2 (methylamine) and 0.38 M CH3NH3Cl (methylammonium…

A: The basic buffer may be explained as the solution mixture which hold the weak base along with its…

Q: Determine the pH of a solution made of 0.0082M H3PO4 and 0.0046M Na2HPO4. (Ka of H3PO4 = 7.11 x…

A: Balance chemical equation:                                   H3PO4 + Na2HPO4  ----->   2NaH2PO4…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 10.04. What is the Kb of this base

A:

Q: What is the pH of 100.0 mL of 0.10 M HNO;? nooulos M 005.0s ai nois 01 x 02.1 g CH'COOH What is the…

A: pH = -log [H+]

Q: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa + log ([A–]/[HA])…

A: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa +log[salt][acid]…

Q: Calculate the pH of 0.0858 M NH3 MM NH3: 17.03 Kb = 1,8 x 10-5 Upload your answer and solutions…

A: The molarity of ammonia is = 0.0858 M The dissociation constant of ammonia is = 1.8×10-5 The pH of…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.26. What is the Kb of this base?…

A: Weak base dissociated less in solution

Q: How many grams of NaOH (MW=40.0 g/mole) do you need to add to 50.0 ml of a 0.2 M weak acid HA…

A: Given data contains, Concentration of HA is 0.2 M. Volume is 50.0 mL. Ka is 4×10-6. The moles of HA…

Q: 9. Predict the pH of the resulting solution when we mix 50.0 mL of 0.010 M HClO with 50.0 mL of…

A: We'll answer the first question since the exact one wasn't specified. Please resubmit a new question…

Q: Im doing a lab report on the creation of soap through the saponification process, and am currently…

A: Soap is made by saponification reaction in laboratory. In this method, soap is made by reacting…

Q: The question says "calculate the ph of the solution." It gives the following: 1.00x 10^-1 M…

A: The given solution mixture is a buffer solution of weak acid acetic acid (CH3COOH) and its salt of…

Q: What quantity (moles) of HCl(g) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00?…

A:

Q: What is the approximate pH of a solution formed by mixing 45.0 mL of 0.10M HNO3, 50.0 mL of 0.20M…

A: Given: The volume of HNO3=45.0 mL  Molarity of HNO3=0.10M  Volume of HCl=50.0 mL  Molarity of…

Q: Which pH would change the least if each of the following were diluted by adding

A: The correct answer is C

Q: Write the dissociation equation and ionization constant expression for a 1 M of acetic  acid.…

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Q: c. 10-8 M HNO3 solution? d. a solution containing 12.2 g KOH dissolved in 800 ml solution. e. a…

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Q: If the OH- ion concentration in an aqueous solution at 25.0 C is measured as 3.4 x 10-3M what is the…

A: 1.Given, Concentration of OH- ion = 3.4*10-3M. Ionization constant of water, Kw = 1.0*10-14.…

Q: The value of Kw at 40 °C is 2.92 x 10-14 a. Calculate the [H*] and [OH] in pure water at 40 °C. b.…

A: Calculations (a) Given Kw = 2.92 x 10-14 [H3O+] [OH-] = 2.92 x 10-14 Since the solution is neutral…

Q: Suppose 5.00 g of propanoic acid (HC3H5O2) is dissolved in enough water to yield 100.0 mL of…

A: Molar mass of propanoic acid = 3×12+6×1+2×16=74g/mol Number of moles = massmolar…

Q: Calculate the pOH of a solution that contains 3.9 × 10¬4 M H3O† at 25 °C. 9.59 10.59 0.59 3.41 4.41

A:

Q: The two acid dissociation constants for sulfurous acid, H,SO, are 1.3x10-2 and 6.3x10-8at 25°C. What…

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Q: 15. Calculate the pH of a solution after 28.00 mL of 0.28 M acetic acid with 15.00 mL of 0.11 M…

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Q: Formic acid (HCOOH) has a Ka = 1.8 × 10-4. What is the pH of a 25.00mL sample of 0.205 M formic…

A: Given: Ka = 1.8 × 10-4 [HCOOH] = 0.205 M

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.