Calculate the ph of a 0.150 m solution of koh
WebFeb 5, 2010 · Calculate the pH when 9.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10??) We have an Answer from Expert. WebScience. Chemistry. Chemistry questions and answers. Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)
Calculate the ph of a 0.150 m solution of koh
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WebOct 31, 2024 · Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹) See answer Advertisement Advertisement RasikaC223971 RasikaC223971 pH is a formula that helps chemist to estimate the acidity of a solution. it calculated as: Where [H= Advertisement WebA 20.0-m L sample of 0.150 M K O H is titrated with 0.125 M H C l O 4 solution. Calculate the p H after the following volumes of acid have been added. Part A. 20.0 m L. Express your answer using two decimal places. Part B. ... 20.0 mL x 0.150 M KOH = 3 millimoles KOH (a strong base)0.125 M HClO4 ...
WebCalculate the pOH of a 0.150 M solution of KOH. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. WebThe pH of an acidic solution is 2.11. What is [H⁺]? 7.8 × 10⁻³ M. The pOH of a basic solution is 5.63. What is [OH⁻]? 2.3 × 10⁻⁶ M ... The solution presented in Section 14.3.5 to deal with nonunique search keys added an extra attribute to the search key. What effect could this change have on the height of the B+-tree?
WebA: Given information, pH of aqueous solution at 25°C = 3.80 Formula used : pH + pOH = 14 pH = -log… question_answer Q: Determine the formula of the conjugate base acid: … WebCalculate the pH when 20.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 1 0 − 9) Previous question Next question Chegg Products & Services
WebFind solutions for your homework. ... Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹) Question: Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)
WebApr 4, 2024 · Find an answer to your question Calculate the ph when 20.0 ml of 0.150 m koh is mixed with 20.0 ml of 0.300 m hbro (ka = 2.5 × 10⁻⁹) violamashego7209 violamashego7209 04/04/2024 SAT ... The pH of the solution is 10.74. the pH refers to the hydrogen ion concentration. It is a measure of the acidity of the solution. kit for kids pregnancy pillowWebJun 2, 2016 · Now, after finding the concentration of the hydronium ion, the pH of the solution is determined: pH = −log[H 3O+] pH = −log[1.5 × 10−12] pH = 11.83 Other Method Find the pOH using the concentration of the … kit for smooth operatorWebFeb 26, 2024 · The ph after the following volumes of acid have been added is mathematically given as. pH=1.82. What is the ph value?. Question Parameters: A 20.0-ml sample of 0.150 m koh is titrated with 0.125 m hclo4 solution.. Generally, the equation for the Chemical Reaction is mathematically given as. HClO4+KOH--->KClO4+H20. … kit for making a pin cushionWebCalculate the pH for each case in the titration of 50.0 mL of 0.150 M HClO (aq) with 0.150 M KOH (aq). Use the ionization constant for HClO . What is the pH before addition of any KOH ? kit for servo motor controllerWebA: To calculate the pH of the solution , we would first calculate the final concentration of acetic…. Q: How many grams of ammonium chloride, NH4Cl, would have to be added to exactly 500 mL of 0.10 M NH3…. A: Click to see the answer. Q: Calculate the pH of the following solutions: a) 0.1000 M NaOH, b) 0.1000 M CH3COOH (Ka = 1.8x10–5),…. kit forage puitsWebFind solutions for your homework. ... Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 28.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹) Question: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 28.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹) kit for sewing toolsWebDec 6, 2024 · Sodium hydroxide is a strong base, which means that it dissociates completely in aqueous solution to produce hydroxide anions in a 1:1 mole ratio. NaOH(aq) → Na+ (aq) +OH− (aq) So your solution has. [OH−] = [NaOH] = 0.150 M. Now, the pOH of the solution can be calculated by using. pOH = − log([OH−]) −−−−−−−−−−− ... kit for tc 99m-labeled rbcs